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|---|---|---|---|---|---|---|---|---|---|---|---|
BfpVOfAr1z4BJ7Kp4vA0h | chemistry | surface-chemistry | colloids | An example of solid sol is : | [{"identifier": "A", "content": "Butter"}, {"identifier": "B", "content": "Hair cream"}, {"identifier": "C", "content": "Gem stones"}, {"identifier": "D", "content": "Paint"}] | ["C"] | null | An example of solid sol is gem stones. | mcq | jee-main-2019-online-11th-january-morning-slot | 4,082 |
FZLerdAfYNiY5LAZXus5Z | chemistry | surface-chemistry | colloids | Haemoglobin and gold sol are examples of : | [{"identifier": "A", "content": "positively charged sols"}, {"identifier": "B", "content": "negatively charged sols"}, {"identifier": "C", "content": "Positively and negatively charged sols, respectively \n"}, {"identifier": "D", "content": "negatively and positively charged sols, respectively "}] | ["C"] | null | Haemoglobin $$\buildrel \, \over
\longrightarrow $$ positive sol
<br>Ag $$-$$ sol $$\buildrel \, \over
\longrightarrow $$ negative sol | mcq | jee-main-2019-online-10th-january-evening-slot | 4,083 |
miMFHPOgfCgdem6M1qFFF | chemistry | surface-chemistry | colloids | For coagulation of arsenious sulphate sol, which one of the following salt solution will be most effective ? | [{"identifier": "A", "content": "BaCl<sub>2</sub>"}, {"identifier": "B", "content": "AlCl<sub>3</sub>"}, {"identifier": "C", "content": "NaCl"}, {"identifier": "D", "content": "Na<sub>3</sub>PO<sub>4</sub>"}] | ["B"] | null | Sulphide is $$-$$ve charged colloid.
<br><br>As coagulation is directly proportional to the effective charge, so cation with maximum charge will be most effective for coagulation.
<br><br>Al<sup>3+</sup> > Ba<sup>2+</sup> > Na<sup>+</sup> coagulating power. | mcq | jee-main-2019-online-9th-january-evening-slot | 4,084 |
o77BKzl7ctMOI0a2fI7k9k2k5h2wthc | chemistry | surface-chemistry | colloids | As per Hardy-Schulze formulation, the flocculation values of the following for ferric hydroxide sol are in the
order : | [{"identifier": "A", "content": "AICl<sub>3</sub> > K<sub>3</sub>[Fe(CN)<sub>6</sub>] > K<sub>2</sub>CrO<sub>4</sub> > KBr = KNO<sub>3</sub>"}, {"identifier": "B", "content": "K<sub>3</sub>[Fe(CN)<sub>6</sub>] < K<sub>2</sub>CrO<sub>4</sub> < KBr = KNO<sub>3</sub> = AlCl<sub>3</sub>"}, {"identifier": "C"... | ["B"] | null | Since, Fe(OH)<sub>3</sub> is positively charged sol, hence,
anionic charge will flocculate.
<br><br>As per Hardy Schulze rules coagulation power
of anion follows the order :
<br><br>Fe(CN)<sub>6</sub><sup>3–</sup> $$>$$ CrO<sub>4</sub><sup>2–</sup> $$>$$ Cl<sup>–</sup> = Br<sup>–</sup><sup></sup> = NO<sub>3</sub>... | mcq | jee-main-2020-online-8th-january-morning-slot | 4,085 |
bMfP4Y4lJQ1dG1YCvTjgy2xukft6yw4a | chemistry | surface-chemistry | colloids | Kraft temperature is the temperature : | [{"identifier": "A", "content": "below which the aqueous solution of\ndetergents starts freezing."}, {"identifier": "B", "content": "above which the formation of micelles takes\nplace."}, {"identifier": "C", "content": "below which the formation of micelles takes\nplace."}, {"identifier": "D", "content": "above which t... | ["B"] | null | Above Kraft temperature(T<sub>k</sub>) the formation of
micelles takes place. | mcq | jee-main-2020-online-6th-september-morning-slot | 4,086 |
PJE05lWLOtmyrfjGG1jgy2xukfcfcxjw | chemistry | surface-chemistry | colloids | A sample of red ink (a colloidal suspension) is
prepared by mixing eosin dye, egg white, HCHO
and water. The component which ensures
stability of the ink sample is : | [{"identifier": "A", "content": "HCHO"}, {"identifier": "B", "content": "Water"}, {"identifier": "C", "content": "Eosin dye"}, {"identifier": "D", "content": "Egg white"}] | ["D"] | null | Egg white is used to stabilise the prepared
colloidal sol.of red ink. | mcq | jee-main-2020-online-4th-september-evening-slot | 4,088 |
iNc6gYDQGEIb1ueWhUjgy2xukf925i6p | chemistry | surface-chemistry | colloids | Match the following :<br/><br/>
<style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;border... | [{"identifier": "A", "content": "(i)-(e), (ii)-(c), (iii)-(a), (iv)-(f)"}, {"identifier": "B", "content": "(i)-(d), (ii)-(b), (iii)-(a), (iv)-(e)"}, {"identifier": "C", "content": "(i)-(d), (ii)-(b), (iii)-(e), (iv)-(f)"}, {"identifier": "D", "content": "(i)-(b), (ii)-(c), (iii)-(e), (iv)-(d)"}] | ["A"] | null | Foam $$ \to $$ Froth, whipped cream, soaplather
<br><br>Gel $$ \to $$ Cheese, butter, jellies
<br><br>Aerosol $$ \to $$ smoke dust
<br><br>Emulsion $$ \to $$ milk | mcq | jee-main-2020-online-4th-september-morning-slot | 4,089 |
T60hgImpCTj8NHN886jgy2xukf2cbbyu | chemistry | surface-chemistry | colloids | Tyndall effect is observed when: | [{"identifier": "A", "content": "The diameter of dispersed particles is similar to the wavelenght of light used."}, {"identifier": "B", "content": "The diameter of dispersed particles is much smaller than the wavelength of light used."}, {"identifier": "C", "content": "The diameter of dispersed particles is much larger... | ["A"] | null | Diameter of dispersed particles should not be much smaller than wavelength of light used. | mcq | jee-main-2020-online-3rd-september-morning-slot | 4,091 |
7DVTTROmCYXe7I0Gi6jgy2xukevl5bks | chemistry | surface-chemistry | colloids | Which of the following is used for the
preparation of colloids? | [{"identifier": "A", "content": "Van Arkel Method"}, {"identifier": "B", "content": "Bredig\u2019s Arc Method"}, {"identifier": "C", "content": "Mond Process"}, {"identifier": "D", "content": "Ostwald Process"}] | ["B"] | null | Bredig's arc method is used for the preparation
of colloids. | mcq | jee-main-2020-online-2nd-september-morning-slot | 4,092 |
af4bXu3X9nuI2j0NTU1klusgkob | chemistry | surface-chemistry | colloids | The nature of charge on resulting colloidal particles when FeCl<sub>3</sub> is added to excess of hot water is : | [{"identifier": "A", "content": "neutral"}, {"identifier": "B", "content": "sometimes positive and sometimes negative"}, {"identifier": "C", "content": "positive"}, {"identifier": "D", "content": "negative"}] | ["C"] | null | If FeCl<sub>3</sub> is added to excess of hot water, a positively charged sol of hydrated ferric oxide is
formed due to adsorption of Fe<sup>3+</sup> ions. | mcq | jee-main-2021-online-26th-february-evening-slot | 4,095 |
soDvuluFNOQSeYyXKi1kmiuhemi | chemistry | surface-chemistry | colloids | The INCORRECT statements below regarding colloidal solutions is : | [{"identifier": "A", "content": "The flocculating power of Al<sup>3+</sup> is more than that of Na<sup>+</sup>."}, {"identifier": "B", "content": "A colloidal solutions shows Brownian motion of colloidal particles."}, {"identifier": "C", "content": "An ordinary filter paper can stop the flow of colloidal particles."}, ... | ["C"] | null | Colloidal solutions can pass through ordinary filter paper but cannot pass through a special filter colloidal solution coated paper.
| mcq | jee-main-2021-online-16th-march-evening-shift | 4,096 |
tHwCMwnxJyXFfhTw3M1kmj7b19z | chemistry | surface-chemistry | colloids | A colloidal system consisting of a gas dispersed in a solid is called a/an : | [{"identifier": "A", "content": "foam"}, {"identifier": "B", "content": "aerosol"}, {"identifier": "C", "content": "solid sol"}, {"identifier": "D", "content": "gel"}] | ["C"] | null | A colloidal system consisting of a gas dispersed in
a solid is called a ‘solid sol’.
| mcq | jee-main-2021-online-17th-march-morning-shift | 4,097 |
6KLlwLujiAQmCK4Uom1kmkiqkyg | chemistry | surface-chemistry | colloids | For the coagulation of a negative sol, the species below, that has the highest flocculating power is : | [{"identifier": "A", "content": "Na<sup>+</sup>"}, {"identifier": "B", "content": "Ba<sup>2+</sup>"}, {"identifier": "C", "content": "PO$$_4^{3 - }$$"}, {"identifier": "D", "content": "SO$$_4^{2 - }$$"}] | ["B"] | null | For a negative sol, a positive ion is required for flocculation.
The greater the valence of the flocculating ion added, the greater is its power to cause
precipitation. This is called Hardy-Schulz law.<br><br>
So, Ba<sup>+2</sup> has highest flocculating power.
| mcq | jee-main-2021-online-17th-march-evening-shift | 4,098 |
1krq67ahw | chemistry | surface-chemistry | colloids | The conditions given below are in the context of observing Tyndall effect in colloidal solutions :<br/><br/>(A) The diameter of the colloidal particles is comparable to the wavelength of light used.<br/><br/>(B) The diameter of the colloidal particles is much smaller than the wavelength of light used.<br/><br/>(C) The ... | [{"identifier": "A", "content": "(A) and (E) only"}, {"identifier": "B", "content": "(C) and (D) only"}, {"identifier": "C", "content": "(A) and (D) only"}, {"identifier": "D", "content": "(B) and (E) only"}] | ["A"] | null | The phenomenon of scattering of light by colloidal particles as a result of which the path of the
beam becomes visible is called a tyndall effect. Smaller the diameter and similar the magnitude
of refractive indices, lesser is the scattering and hence the tyndall effect and viced-versa. The
diameter of the dispersed ph... | mcq | jee-main-2021-online-20th-july-morning-shift | 4,100 |
1krrl97jv | chemistry | surface-chemistry | colloids | 100 ml of 0.0018% (w/v) solution of Cl<sup>$$-$$</sup> ion was the minimum concentration of Cl<sup>$$-$$</sup> required to precipitate a negative sol in one h. The coagulating value of Cl<sup>$$-$$</sup> ion is _________ (Nearest integer) | [] | null | 1 | Coagulation value The minimum concentration of electrolyte in millimoles required to cause coagulation of 1 L of colloidal solution. <br/><br/>Given, 0.0018 g Cl<sup>$$-$$</sup> present in 100 mL solution<br/><br/>Coagulation value of Cl<sup>$$-$$</sup> is $$ = {{{{0.0018} \over {35.5}} \times {{10}^3}} \over {0.1}} = ... | integer | jee-main-2021-online-20th-july-evening-shift | 4,101 |
1krxb2oy9 | chemistry | surface-chemistry | colloids | Match List I with List II :<br/><br/><table style="width: 100%">
<thead>
<tr>
<th>List-I<br/>Example of colloids</th>
<th>List - II<br/>Classification</th>
</tr>
</thead>
<tbody>
<tr>
<td>(a) Cheese</td>
<td>(i) dispersion of liquid in liquid</td>
</tr>
<tr>
<td>(b) Pumice stone</td>
<td>(ii) dispersion of liquid in g... | [{"identifier": "A", "content": "(a)-(iv), (b)-(iii), (c)-(ii), (d)-(i)"}, {"identifier": "B", "content": "(a)-(iv), (b)-(i), (c)-(iii), (d)-(ii)"}, {"identifier": "C", "content": "(a)-(iii), (b)-(iv), (c)-(i), (d)-(ii)"}, {"identifier": "D", "content": "(a)-(iv), (b)-(iii), (c)-(i), (d)-(ii)"}] | ["D"] | null | Cheese $$\to$$ liquid in solid<br><br>Pumice stone $$\to$$ gas in solid<br><br>Hair cream $$\to$$ liquid in liquid<br><br>Cloud $$\to$$ liquid in gas | mcq | jee-main-2021-online-25th-july-evening-shift | 4,102 |
1ktcp1mny | chemistry | surface-chemistry | colloids | The sol given below with negatively charged colloidal particles is : | [{"identifier": "A", "content": "FeCl<sub>3</sub> added to hot water"}, {"identifier": "B", "content": "KI added to AgNO<sub>3</sub> solution"}, {"identifier": "C", "content": "AgNO<sub>3</sub> added to KI solution"}, {"identifier": "D", "content": "Al<sub>2</sub>O<sub>3</sub>.xH<sub>2</sub>O in water"}] | ["C"] | null | <p>When AgNO<sub>3</sub>
is added to KI,</p>
<img src="https://app-content.cdn.examgoal.net/fly/@width/image/1l09tqvxx/7f6d0d46-03ce-4be5-9a34-f82e5b2c2e07/0042a650-9a4d-11ec-bb3a-6b144b885005/file-1l09tqvxy.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1l09tqvxx/7f6d0d46-03ce-4be5-9a34-f82e5b2... | mcq | jee-main-2021-online-26th-august-evening-shift | 4,103 |
1ktecswl2 | chemistry | surface-chemistry | colloids | Tyndall effect is more effectively shown by : | [{"identifier": "A", "content": "true solution"}, {"identifier": "B", "content": "lyophilic colloid"}, {"identifier": "C", "content": "lyophobic colloid"}, {"identifier": "D", "content": "suspension"}] | ["C"] | null | Tyndall effect is observed in lyophobic colloids | mcq | jee-main-2021-online-27th-august-morning-shift | 4,104 |
1ktfsenzv | chemistry | surface-chemistry | colloids | Lyophilic sols are more stable than lyophobic sols because : | [{"identifier": "A", "content": "there is a strong electrostatic repulsion between the negatively charged colloidal particles."}, {"identifier": "B", "content": "the colloidal particles have positive charge."}, {"identifier": "C", "content": "the colloidal particles have no charge."}, {"identifier": "D", "content": "th... | ["D"] | null | In the lyophilic colloids, the colloidal particles are extensively solvated. | mcq | jee-main-2021-online-27th-august-evening-shift | 4,105 |
1ktn0dtf9 | chemistry | surface-chemistry | colloids | Match List - I with List - II :<br/><br/>
<img src="data:image/png;base64,UklGRtJAAABXRUJQVlA4IMZAAAAw8gCdASoAA84APm00lUekIyIhJDI8GIANiWlu/HyZUcADOzrp/TX+of1n9f/AL+7/4H9qv7f6U/jHy392/t/+Q/3/949uv/A79/oX8j/z/Qz+Q/Zj8h/c/8T/3/8J7X/5X/IfjZ6D/mH7X/r/tz+QX8l/nf+O/vf5F+pX/h9rxtv+v/7nqC+rP03/Z/5L/Pfs96J/+D/f/8V7E/oP+B/5H9/+AH... | [{"identifier": "A", "content": "(a)-(i), (b)-(iii), (c)-(ii), (d)-(iv)"}, {"identifier": "B", "content": "(a)-(iv), (b)-(i), (c)-(iii), (d)-(ii)"}, {"identifier": "C", "content": "(a)-(iv), (b)-(ii), (c)-(iii), (d)-(i)"}, {"identifier": "D", "content": "(a)-(i), (b)-(ii), (c)-(iv), (d)-(iii)"}] | ["B"] | null | In reaction (i), Au (sol) is formed by reduction of
AuCl<sub>3</sub>, so the chemical method of preparation is
“Reduction”.
<br><br>In reaction (ii), As<sub>2</sub>S<sub>3</sub> (sol) is formed by double
decomposition, so the chemical method of
preparation is “Double decomposition”.
<br><br>In reaction (iii), S (sol) i... | mcq | jee-main-2021-online-1st-september-evening-shift | 4,106 |
1l54y6j4t | chemistry | surface-chemistry | colloids | <p>A 42.12% (w/v) solution of NaCl causes precipitation of a certain sol in 10 hours. The coagulating value of NaCl for the sol in 2 hours is :</p>
<p>[Given : Molar mass : Na = 23.0 g mol<sup>$$-$$1</sup> ; Cl = 35.5 g mol<sup>$$-$$1</sup>]</p> | [{"identifier": "A", "content": "36 m mol L<sup>$$-$$1</sup>"}, {"identifier": "B", "content": "36 mol L<sup>$$-$$1</sup>"}, {"identifier": "C", "content": "1440 mol L<sup>$$-$$1</sup>"}, {"identifier": "D", "content": "1440 m mol L<sup>$$-$$1</sup>"}] | ["D"] | null | Data is insufficient. | mcq | jee-main-2022-online-29th-june-evening-shift | 4,108 |
1l56aj493 | chemistry | surface-chemistry | colloids | <p>The Zeta potential is related to which property of colloids?</p> | [{"identifier": "A", "content": "Colour"}, {"identifier": "B", "content": "Tyndall effect"}, {"identifier": "C", "content": "Charge on the surface of colloidal particles"}, {"identifier": "D", "content": "Brownian movement"}] | ["C"] | null | The potential difference between the fixed layer and
the diffused layer of opposite charges is called zeta
potential.<br/><br/>
It is related to the charge on the surface of colloidal particles. | mcq | jee-main-2022-online-28th-june-morning-shift | 4,110 |
1l57rl0bt | chemistry | surface-chemistry | colloids | <p>Match List-I with List-II</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;bo... | [{"identifier": "A", "content": "(A) - (II), (B) - (I), (C) - (IV), (D) - (III)"}, {"identifier": "B", "content": "(A) - (III), (B) - (I), (C) - (IV), (D) - (II)"}, {"identifier": "C", "content": "(A) - (II), (B) - (I), (C) - (III), (D) - (IV)"}, {"identifier": "D", "content": "(A) - (III), (B) - (II), (C) - (I), (D) -... | ["A"] | null | (A) Protective colloids are lyophilic colloids<br/><br/>
(B) Emulsions are liquid in liquid colloidal
solutions<br/><br/>
(C) FeCl<sub>3</sub> + hot water forms positively charged
colloidal solution of hydrated ferric oxide.<br/><br/>
(D) FeCl<sub>3</sub> + NaOH forms negatively charged
colloidal solution due to pre... | mcq | jee-main-2022-online-27th-june-morning-shift | 4,111 |
1l5almtuu | chemistry | surface-chemistry | colloids | <p>Incorrect statement for Tyndall effect is :</p> | [{"identifier": "A", "content": "The refractive indices of the dispersed phase and the dispersion medium differ greatly in magnitude."}, {"identifier": "B", "content": "The diameter of the dispersed particles is much smaller than the wavelength of the light used."}, {"identifier": "C", "content": "During projection of ... | ["B"] | null | For Tyndall effect, the diameter of the dispersed
particles is not much smaller than the wavelength
of the light used. | mcq | jee-main-2022-online-25th-june-morning-shift | 4,112 |
1l5ama29a | chemistry | surface-chemistry | colloids | <p>Using very little soap while washing clothes, does not serve the purpose of cleaning of clothes, because :</p> | [{"identifier": "A", "content": "soap particles remain floating in water as ions."}, {"identifier": "B", "content": "the hydrophobic part of soap is not able to take away grease."}, {"identifier": "C", "content": "the micelles are not formed due to concentration of soap, below its CMC value."}, {"identifier": "D", "con... | ["C"] | null | The little amount of using soap while washing
clothes, does not serve the purpose of cleaning of
clothes because the micelles are not formed due to
the low concentration of soap as it is below CMC. | mcq | jee-main-2022-online-25th-june-morning-shift | 4,113 |
1l5c6bsns | chemistry | surface-chemistry | colloids | <p>Given below are two statements :</p>
<p>Statement I : Emulsions of oil in water are unstable and sometimes they separate into two layers on standing.</p>
<p>Statement II : For stabilisation of an emulsion, excess of electrolyte is added.</p>
<p>In the light of the above statements, choose the most appropriate answer... | [{"identifier": "A", "content": "Both Statement I and Statement II are correct."}, {"identifier": "B", "content": "Both Statement I and Statement II are incorrect."}, {"identifier": "C", "content": "Statement I is correct but Statement II is incorrect."}, {"identifier": "D", "content": "Statement I is incorrect but Sta... | ["C"] | null | Oil in water emulsions can sometimes separate into
two layers on standing.<br/><br/>
The most relevant example for the above case is
milk, which can separate into two layers on
standing for a longer time. Therefore, statement (I)
is correct.<br/><br/>
On adding excess of electrolyte, coagulation occurs
and emulsion is ... | mcq | jee-main-2022-online-24th-june-morning-shift | 4,114 |
1l6kpa2gm | chemistry | surface-chemistry | colloids | <p>Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).</p>
<p>Assertion (A) : Dissolved substances can be removed from a colloidal solution by diffusion through a parchment paper.</p>
<p>Reason (R) : Particles in a true solution cannot pass through parchment paper ... | [{"identifier": "A", "content": "Both (A) and (R) are correct and (R) is the correct explanation of (A)"}, {"identifier": "B", "content": "Both (A) and (R) are correct but (R) is not the correct explanation of (A)"}, {"identifier": "C", "content": "(A) is correct but (R) is not correct"}, {"identifier": "D", "content":... | ["C"] | null | Parchment paper is a semi-permeable membrane which allows particles of true solution to pass through as their size are too small.
<br/><br/>
Assertion is correct but reason is incorrect. | mcq | jee-main-2022-online-27th-july-evening-shift | 4,118 |
1l6p6wgu2 | chemistry | surface-chemistry | colloids | <p>$$100 \mathrm{~mL}$$ of $$5 \%\,(\mathrm{w} / \mathrm{v})$$ solution of $$\mathrm{NaCl}$$ in water was prepared in $$250 \mathrm{~mL}$$ beaker. Albumin from the egg was poured into $$\mathrm{NaCl}$$ solution and stirred well. This resulted in a/an :</p> | [{"identifier": "A", "content": "Lyophilic sol"}, {"identifier": "B", "content": "Lyophobic sol"}, {"identifier": "C", "content": "Emulsion"}, {"identifier": "D", "content": "Precipitate"}] | ["A"] | null | Albumin from the egg was poured into $100 \mathrm{~mL}$ of $5 \%$ (w/v) $\mathrm{NaCl}$ solution in water. This would result in the formation of lyophilic sol. Albumin molecules get dispersed in water the colloidal particles of albumin are stabilised by hydrogen bond with water molecules. | mcq | jee-main-2022-online-29th-july-morning-shift | 4,119 |
1ldpp0eww | chemistry | surface-chemistry | colloids | <p>Adding surfactants in non polar solvent, the micelles structure will look like</p>
<p><img src="data:image/png;base64,UklGRv4UAABXRUJQVlA4IPIUAACQwACdASoAAyQBP4G40mO2LasmpJJ6usAwCWlu/EsYEY3HZ18/rN/vv7P3q+A9fyz/9Zn993x74f/d7xCAT78cZP3t2Aw3tj9kK6OY9Q5Cprol3QPb3vcNqBbEzYB4q8d5D5n1E3R9y4CvLF4xMLYUmddWsTP4CUl8pL5SXykvlJf... | [{"identifier": "A", "content": "d"}, {"identifier": "B", "content": "a"}, {"identifier": "C", "content": "c"}, {"identifier": "D", "content": "b"}] | ["B"] | null | Non-Polar tail towards non-polar solvent. | mcq | jee-main-2023-online-31st-january-morning-shift | 4,120 |
1ldr4e1fd | chemistry | surface-chemistry | colloids | <p>Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).</p>
<p>Assertion (A) : In expensive scientific instruments, silica gel is kept in watch-glasses or in semipermeable membrane bags.</p>
<p>Reason (R) : Silica gel adsorbs moisture from air via adsorption, thus p... | [{"identifier": "A", "content": "Both (A) and (R) are true and (R) is the correct explanation of (A)"}, {"identifier": "B", "content": "(A) is true but (R) is false"}, {"identifier": "C", "content": "(A) is false but (R) is true"}, {"identifier": "D", "content": "Both (A) and (R) are true but (R) is not the correct exp... | ["A"] | null | <p>Assertion is correct and Reason is correct explanation of Assertion.</p>
<p>Silica gel adsorbs moisture and thus products the instrument from water corrosion (rusting) and prevents malfunctioning.</p> | mcq | jee-main-2023-online-30th-january-morning-shift | 4,121 |
1ldscohtd | chemistry | surface-chemistry | colloids | <p>Match List I and List II</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;bor... | [{"identifier": "A", "content": "A-III, B-I, C-IV, D-II"}, {"identifier": "B", "content": "A-III, B-I, C-II, D-IV"}, {"identifier": "C", "content": "A-I, B-III, C-IV, D-II"}, {"identifier": "D", "content": "A-I, B-III, C-II, D-IV"}] | ["A"] | null | <p>Correct match is :</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;border-wi... | mcq | jee-main-2023-online-29th-january-evening-shift | 4,122 |
1ldss2vd1 | chemistry | surface-chemistry | colloids | <p>Which of the following salt solutions would coagulate the colloid solution formed when $$\mathrm{FeCl_3}$$ is added to $$\mathrm{NaOH}$$ solution, at the fastest rate?</p> | [{"identifier": "A", "content": "10 mL of 0.15 mol dm$$^{-3}$$ CaCl$$_2$$"}, {"identifier": "B", "content": "10 mL of 0.2 mol dm$$^{-3}$$ AlCl$$_3$$"}, {"identifier": "C", "content": "10 mL of 0.1 mol dm$$^{-3}$$ Na$$_2$$SO$$_4$$"}, {"identifier": "D", "content": "10 mL of 0.1 mol dm$$^{-3}$$ Ca$$_3$$(PO$$_4$$)$$_2$$"}... | ["B"] | null | In the coagulation of a negative sol, the flocculating power is in the order.
<br/><br/>
$\therefore \mathrm{Al}^{3+}>\mathrm{Ba}^{2+}>\mathrm{Na}^{+}$and $\mathrm{FeCl}_{3}$ with $\mathrm{NaOH}$ forms a negative sol.
<br/><br/>
$\therefore \mathrm{AlCl}_{3}$ coagulate it most. | mcq | jee-main-2023-online-29th-january-morning-shift | 4,123 |
1ldu1g5zi | chemistry | surface-chemistry | colloids | <p>Based on the given figure, the number of <b>correct</b> statement/s is/are __________.</p>
<p><img src="data:image/png;base64,UklGRq4ZAABXRUJQVlA4IKIZAADQGQGdASoAA/EBP4G21WW2LSunIVBKSsAwCWlu8p9XvMv+LDRkpr+dv9V/hPZf1L2tzBn810f/Wv/d/sP48/M33/9wjr24NUAH3d9C7/7xr//mzbnlP/31Afu//4FdOE/JO7u7u7u7u7u7u7u7u7u7u7u7u7unFnoCSCm... | [] | null | 2 | The correct statements are<br/><br/>
(B) Surface tension is due to uneven forces acting on the molecules present on the surface<br/><br/>
(D) The molecules on the surface are responsible for vapor pressure if the system is a closed system | integer | jee-main-2023-online-25th-january-evening-shift | 4,124 |
1ldyfpgfp | chemistry | surface-chemistry | colloids | <p>Statement I : For colloidal particles, the values of colligative properties are of small order as compared to values shown by true solutions at same concentration.</p>
<p>Statement II : For colloidal particles, the potential difference between the fixed layer and the diffused layer of same charges is called the elec... | [{"identifier": "A", "content": "Both Statement I and Statement II are false"}, {"identifier": "B", "content": "Statement I is true and Statement II is false"}, {"identifier": "C", "content": "Both Statement I and Statement II are true"}, {"identifier": "D", "content": "Statement I is false but Statement II is true"}] | ["B"] | null | <p><b>Statement I: </b>For colloidal particles, the values of colligative properties are of small order as compared to values shown by true solutions at the same concentration.</p>
<p>This statement is true. Colloidal particles are intermediate in size between true solutions and suspensions, and their properties diffe... | mcq | jee-main-2023-online-24th-january-morning-shift | 4,125 |
lgo0dn3e | chemistry | surface-chemistry | colloids | $20 \mathrm{~mL}$ of $0.5 \mathrm{M} ~\mathrm{NaCl}$ is required to coagulate $200 \mathrm{~mL}$ of $\mathrm{As}_{2} \mathrm{S}_{3}$ solution in 2 hours. The coagulating value of $\mathrm{NaCl}$ is ____________ . | [] | null | 50 | The coagulating value of an electrolyte is defined as the minimum amount of the electrolyte required to coagulate a unit volume of the colloidal solution in a given time. In this problem, we are given that $20\ \mathrm{mL}$ of $0.5\ \mathrm{M}$ $\mathrm{NaCl}$ solution is required to coagulate $200\ \mathrm{mL}$ of $\m... | integer | jee-main-2023-online-15th-april-morning-shift | 4,126 |
1lgp2rny4 | chemistry | surface-chemistry | colloids | <p>Given below are two statements, one is labelled as Assertion A and the other is labelled as Reason R.</p>
<p>Assertion A : The diameter of colloidal particles in solution should not be much smaller than wavelength of light to show Tyndall effect.</p>
<p>Reason R : The light scatters in all directions when the size o... | [{"identifier": "A", "content": "Both A and R are correct and R is the correct explanation of A"}, {"identifier": "B", "content": "A is true but R is false"}, {"identifier": "C", "content": "Both A and R are correct but R is NOT the correct explanation of A"}, {"identifier": "D", "content": "A is false but R is true"}] | ["A"] | null | Tyndall effect is observed only when the following two conditions are satisfied<br/><br/>
(a) The diameter of the dispersed particle is not much smaller than the wave length of light used.<br/><br/>
(b) Refractive indices of dispersed phase and dispersion medium differ greatly in magnitude. | mcq | jee-main-2023-online-13th-april-evening-shift | 4,127 |
1lgvtv38n | chemistry | surface-chemistry | colloids | <p>Ferric chloride is applied to stop bleeding because -</p> | [{"identifier": "A", "content": "$$\\mathrm{FeCl}_{3}$$ reacts with the constituents of blood which is a positively charged sol."}, {"identifier": "B", "content": "Blood absorbs $$\\mathrm{FeCl}_{3}$$ and forms a complex."}, {"identifier": "C", "content": "$$\\mathrm{Cl}^{-}$$ ions cause coagulation of blood."}, {"iden... | ["D"] | null | <p>The correct answer is <strong>Option D: Fe<sup>3+</sup> ions coagulate blood which is a negatively charged sol.</strong></p>
<p>Blood is a colloidal solution, which means that it is made up of small particles suspended in a liquid. The particles in blood are negatively charged, and the negative charge prevents the p... | mcq | jee-main-2023-online-10th-april-evening-shift | 4,129 |
1lgyson52 | chemistry | surface-chemistry | colloids | <p>Coagulating value of the electrolytes $$\mathrm{AlCl}_{3}$$ and $$\mathrm{NaCl}$$ for $$\mathrm{As}_{2} \mathrm{S}_{3}$$ are 0.09 and 50.04 respectively. The coagulating power of $$\mathrm{AlCl}_{3}$$ is $$x$$ times the coagulating power of $$\mathrm{NaCl}$$. The value of $$\underline{x}$$ is ___________.</p> | [] | null | 556 | <p>The coagulating power of an electrolyte is inversely proportional to its coagulating value. That is,</p>
<p>$$
\text{Coagulating power} = \frac{1}{\text{Coagulating value}}
$$</p>
<p>Therefore, the coagulating power of AlCl₃ is $$
\frac{1}{0.09}
$$</p>
<p>and the coagulating power of NaCl is $$
\frac{1}{50.04}
$$</p... | integer | jee-main-2023-online-8th-april-evening-shift | 4,130 |
phalQRQ972Brggx5 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point, then : | [{"identifier": "A", "content": "$$\\Delta H$$ is -ve, $$\\Delta S$$ is +ve"}, {"identifier": "B", "content": "$$\\Delta H$$ and $$\\Delta S$$ are both +ve"}, {"identifier": "C", "content": "$$\\Delta H$$ and $$\\Delta S$$ are both -ve"}, {"identifier": "D", "content": "$$\\Delta H$$ is +ve, $$\\Delta S$$ is -ve"}] | ["B"] | null | <b>TIPS/Formulae :</b>
<br><br>$$\Delta G = \Delta H - T\Delta S$$
<br><br>Since $$\Delta G = \Delta H - T\Delta S$$ for an endothermic reaction,
<br><br>$$\Delta H = + ve$$ and at low temperature $$\Delta S = + ve$$
<br><br>Hence $$\Delta G = \left( + \right)\Delta H - T\left( + \right)\Delta S$$
<br><br>and i... | mcq | aieee-2002 | 4,132 |
sPSvpoqLxuJ2aurO | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | In an irreversible process taking place at constant T and P and in which only pressure-volume work is being done, the change in Gibbs free energy (dG) and change in entropy (dS), satisfy the criteria : | [{"identifier": "A", "content": "(dS)<sub>V, E</sub> > 0, (dG)<sub>T, P</sub> < 0"}, {"identifier": "B", "content": "(dS)<sub>V, E</sub> = 0, (dG)<sub>T, P</sub> = 0"}, {"identifier": "C", "content": "(dS)<sub>V, E</sub> = 0, (dG)<sub>T, P</sub> > 0"}, {"identifier": "D", "content": "(dS)<sub>V, E</sub> < 0... | ["A"] | null | For spontaneous reaction, $$dS > 0$$ and $$dG$$ should be negative i.e. $$ < 0.$$ | mcq | aieee-2003 | 4,133 |
sHDrywGF2oZGYLEv | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The correct relationship between free energy change in a reaction and the corresponding equilibrium constant K<sub>c</sub> is : | [{"identifier": "A", "content": "- $$\\Delta G$$ = RT ln K<sub>c</sub>"}, {"identifier": "B", "content": "$$\\Delta G^o$$ = RT ln K<sub>c</sub>"}, {"identifier": "C", "content": "- $$\\Delta G^o$$ = RT ln K<sub>c</sub>"}, {"identifier": "D", "content": "$$\\Delta G$$ = RT ln K<sub>c</sub>"}] | ["C"] | null | $$\Delta {G^ \circ } = - RT\,1n{K_c}\,\,\,$$ or $$\,\,\, - \Delta {G^ \circ } = RT\,1n{K_c}$$ | mcq | aieee-2003 | 4,134 |
QIZvwTiW2R9ZxNa5 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | In conversion of lime-stone to lime, <br/>
CaCO<sub>3</sub>(s) $$\to$$ CaO(s) + CO<sub>2</sub> (g) the vales of ∆H° and ∆S° are +179.1 kJ mol−1
and 160.2 J/K respectively at 298 K and 1 bar.
Assuming that ∆H° do not change with temperature, temperature above which conversion of
limestone to lime will be spontaneous is... | [{"identifier": "A", "content": "1008 K "}, {"identifier": "B", "content": "1200 "}, {"identifier": "C", "content": "845 K"}, {"identifier": "D", "content": "1118 K "}] | ["D"] | null | $$\Delta {G^ \circ } = \Delta {H^ \circ } - T\Delta {S^ \circ }$$
<br><br>For a spontaneous reaction $$\Delta {G^ \circ } < 0$$
<br><br>or $$\,\,\,\Delta {H^ \circ } - T\Delta {S^ \circ } < 0$$
<br><br>$$ \Rightarrow T > {{\Delta {H^ \circ }} \over {\Delta {S^ \circ }}}$$
<br><br>$$ \Rightarrow T > {{179.3... | mcq | aieee-2007 | 4,135 |
6wcnWh2dejd5kT3l | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | Standard entropy of X<sub>2</sub>, Y<sub>2</sub> and XY<sub>3</sub> are 60, 40 and 50 JK<sup>−1</sup>
mol<sup>−1</sup> , respectively. For the reaction, <br/>
$${1 \over 2} X_2$$ + $${3 \over 2} Y_2 \to$$ XY<sub>3</sub>, $$\Delta H$$ = -30 kJ, to be at equilibrium, the temperature will be : | [{"identifier": "A", "content": "1250 K"}, {"identifier": "B", "content": "500 K"}, {"identifier": "C", "content": "750 K"}, {"identifier": "D", "content": "1000 K"}] | ["C"] | null | For a reaction to be at equilibrium $$\Delta G = 0.$$
<br><br>Since $$\Delta G = \Delta H - T\Delta S$$
<br><br>so at equilibrium $$\Delta H - T\Delta S = 0$$
<br><br>or $$\,\,\,\,\Delta H = T\Delta S$$
<br><br>For the reaction
<br><br>$${1 \over 2}{X_2} + {3 \over 2}{Y_2} \to X{Y_3};\,\,\,$$
<br><br>$$\Delta H ... | mcq | aieee-2008 | 4,136 |
8YOhXpsnxnaq1ymO | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For a particular reversible reaction at temperature T, ∆H and ∆S were found to be both +ve. If T<sub>e</sub> is
the temperature at equilibrium, the reaction would be spontaneous when : | [{"identifier": "A", "content": "T<sub>e</sub> > T"}, {"identifier": "B", "content": "T > T<sub>e</sub>"}, {"identifier": "C", "content": "T<sub>e</sub> is 5 times T"}, {"identifier": "D", "content": "T = T<sub>e</sub>"}] | ["B"] | null | At equilibrium $$\Delta G = 0$$
<br><br>Hence, $$\Delta G = \Delta H - {T_e}\Delta S = 0$$
<br><br>$$\therefore$$ $$\,\,\,\,\,\,\Delta H = {T_e}\Delta S\,\,\,$$
<br><br>or $$\,\,\,\,{T_e} = {{\Delta H} \over {\Delta S}}\,\,$$
<br><br>For a spontaneous reaction
<br><br>$$\Delta G$$ must be negative
<br><br>which is ... | mcq | aieee-2010 | 4,137 |
BcphWoKO63fYQVqB | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a
volume of 10 dm<sup>3</sup> to a volume of 100 dm<sup>3</sup> at 27<sup>o</sup>C is : | [{"identifier": "A", "content": "35.8 J mol<sup>-1</sup> K<sup>\u22121</sup> "}, {"identifier": "B", "content": "32.3 J mol<sup>-1</sup> K<sup>\u22121</sup> "}, {"identifier": "C", "content": "42.3 J mol<sup>-1</sup> K<sup>\u22121</sup> "}, {"identifier": "D", "content": "38.3 J mol<sup>-1</sup> K<sup>\u22121</sup> "}] | ["D"] | null | Entropy change for an isothermal reversible process is given by
<br><br>$$\Delta S = nR{\mkern 1mu} ln{{{V_2}} \over {{V_1}}}$$
<br><br>$$ = 2 \times 8.314 \times 2.303log\,{{100} \over {10}}$$
<br><br>$$ = 38.3\,J\,mo{l^{ - 1}}\,\,{K^{ - 1}}$$ | mcq | aieee-2011 | 4,138 |
eaqqbvY65NgoNa5n | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The incorrect expression among the following is : | [{"identifier": "A", "content": "$${{\\Delta {G_{system}}} \\over {\\Delta {S_{total}}}} = - T$$ "}, {"identifier": "B", "content": "In isothermal process $${w_{reversible}}$$ = $$ - nRT\\,\\ln \\,{{{V_f}} \\over {{V_i}}}$$"}, {"identifier": "C", "content": "In $$K\\, = {{\\Delta {H^o} - T\\Delta {S^o}} \\over {RT}}$$... | ["C"] | null | $$\Delta {G^ \circ } = \Delta {H^ \circ } - T\Delta {S^ \circ };$$
<br><br>$$\,\,\,\,\,\,\,\,\, - RT\,\ell nK = \Delta {H^ \circ } - T\Delta {S^ \circ }$$
<br><br>$$\ell nK = - {{\Delta {H^ \circ } - T\Delta {S^ \circ }} \over {RT}}$$ | mcq | aieee-2012 | 4,139 |
abw0HPkOJTHzb9O6 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The following reaction is performed at 298 K<br/>
2NO(g) + O<sub>2</sub> (g) $$\leftrightharpoons$$ 2NO<sub>2</sub> (g)<br/>
The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy
of formation of NO<sub>2</sub>(g) at 298 K? (KP = 1.6 × 10<sup>12</sup>) | [{"identifier": "A", "content": "86600 + R(298) ln(1.6 $$\\times$$ 10<sup>12</sup>)"}, {"identifier": "B", "content": "86600 - $$ln (1.6 \\times 10^{12}) \\over R (298)$$"}, {"identifier": "C", "content": "0.5[2\u00d786,600 \u2013 R(298) ln(1.6\u00d710<sup>12</sup>)] "}, {"identifier": "D", "content": "R(298) ln(1.6\u0... | ["C"] | null | $$\Delta {G^ \circ }_{NO\left( g \right)}$$
<br><br>$$\,\,\,\,\,\,\,\,\,\,\,\,\, = 86.6kJ/mol = 86600J/mol;$$
<br><br>$$\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,$$$${G^ \circ }_{N{O_2}\left( g \right)} = x\,J/mol$$
<br><br>$$T = 298,\,{K_p} = 1.6 \times {10^{12}}$$
<br><br>$$\Delta {G^ \circ } = - RT\,\ln \,{K_p}$$
<br><br>Giv... | mcq | jee-main-2015-offline | 4,140 |
zpIcoQr9rindaITQXyhpP | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The plot shows the variation of −$$ln$$ K<sub>p</sub> versus temperature for the two reactions.
<br/><br/>M(s) + $${1 \over 2}$$ O<sub>2</sub>(g) $$ \to $$ MO(s) and
<br/><br/>C(s) + $${1 \over 2}$$ O<sub>2</sub>(g) $$ \to $$ CO(s)
<br/><br/><img src="data:image/png;base64,UklGRnIPAABXRUJQVlA4IGYPAABw3ACdASoAAx0CP4G+1... | [{"identifier": "A", "content": "At T > 1200 K, carbon will reduce MO(s) to M(s)."}, {"identifier": "B", "content": "At T < 1200 K, the reaction \n<br><br>MO(s) + C(s) $$ \\to $$ M(s) + CO(g) is spontaneous."}, {"identifier": "C", "content": "At T < 1200 K, oxidation of carbon is unfavourable"}, {"identifier"... | ["B"] | null | <p>Carbon is a good reducing agent for oxides. The reason why carbon reduces metal oxide spontaneously at T < 1200 K is that $$ - {{\ln {K_p}} \over T}$$ line for CO has a negative slope.</p> | mcq | jee-main-2016-online-9th-april-morning-slot | 4,141 |
QV1uDvUN2q3sFjXdOuRMm | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous
at high temperature. Identify the correct statement about the reaction among the
following : | [{"identifier": "A", "content": "Both $$\\Delta $$H and $$\\Delta $$S are negative."}, {"identifier": "B", "content": "Both $$\\Delta $$H and $$\\Delta $$S are positive."}, {"identifier": "C", "content": "$$\\Delta $$H is positive while $$\\Delta $$S is negative."}, {"identifier": "D", "content": "$$\\Delta $$H is nega... | ["B"] | null | <p>We know that $$\Delta$$G = $$\Delta$$H $$-$$ T$$\Delta$$S</p>
<p>At low temperature : $$\Delta$$G is positive (non-spontaneous process), so $$\Delta$$H is positive and $$\Delta$$S is positive (T$$\Delta$$S < $$\Delta$$H as T is low).</p>
<p>At high temperature : $$\Delta$$G is negative (spontaneous process), so $$\D... | mcq | jee-main-2016-online-9th-april-morning-slot | 4,142 |
iaIfEPNoZEMepV4TiITWS | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For the reaction,
<br/>A(g) + B(g) $$ \to $$ C(g) + D(g), $$\Delta $$H<sup>o</sup> and $$\Delta $$S<sup>o</sup> are, respectively, − 29.8 kJ mol<sup>−1</sup> and −0.100 kJ K<sup>−1</sup> mol<sup>−1</sup> at 298 K. The equilibrium constant for the reaction at 298 K is : | [{"identifier": "A", "content": "1.0 $$ \\times $$ 10<sup>$$-$$10</sup>"}, {"identifier": "B", "content": "1.0 $$ \\times $$ 10<sup>10</sup>"}, {"identifier": "C", "content": "10"}, {"identifier": "D", "content": "1"}] | ["D"] | null | <p>We have</p>
<p>$$\Delta$$G$$^\circ$$ = $$\Delta$$H$$^\circ$$ $$-$$ T$$\Delta$$S$$^\circ$$</p>
<p>$$\Delta$$G$$^\circ$$ = $$-$$ 29.8 $$-$$ 298 ($$-$$ 0.1) = 0</p>
<p>$$\Delta$$G$$^\circ$$ = $$-$$ 2.302 RT log K<sub>eq</sub></p>
<p>log K<sub>eq</sub> = 0 $$\Rightarrow$$ K<sub>eq</sub> = 1</p> | mcq | jee-main-2016-online-9th-april-morning-slot | 4,143 |
3oMCAaXlAkKhZuVDEwROx | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | At 320 K, a gas A<sub>2</sub> is 20% dissociated to A(g). The standard free energy change at 320 K and 1 atm in J mol<sup>-1</sup> is approximately : (R = 8.314 JK<sup>-1</sup> mol<sup>-1</sup>; ln2 = 0.693; ln 3 = 1.098) | [{"identifier": "A", "content": "4763"}, {"identifier": "B", "content": "2068"}, {"identifier": "C", "content": "1844"}, {"identifier": "D", "content": "4281"}] | ["D"] | null | A<sub>2</sub> (g) $$\rightleftharpoons$$ 2 A (g)
<br><br>Assume initially concentration of A<sub>2</sub> = [A<sub>2</sub>] = 1 m
<br><br>at equilibrium [A<sub>2</sub>] = 1 $$ \times $$ $${{80} \over {100}}$$ = 0.8 M
<br><br>and 20% of [A<sub>2</sub>] = 1 $$ \times $$ $${{20} \over {100}}$$ = 0.2 M
<br><br>$$\therefore... | mcq | jee-main-2018-online-16th-april-morning-slot | 4,144 |
QRNOQ7ZCfVfwo5d0EfXXZ | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For which of the following processes, $$\Delta $$S is negative ? | [{"identifier": "A", "content": "H<sub>2</sub>(g) $$ \\to $$ 2H(g)"}, {"identifier": "B", "content": "N<sub>2</sub>(g, 1 atm) $$ \\to $$ N<sub>2</sub>(g, 5 atm)"}, {"identifier": "C", "content": "C(diamond) $$ \\to $$ C(graphite)"}, {"identifier": "D", "content": "N<sub>2</sub>(g, 273 K) $$ \\to $$ N<sub>2</sub>(... | ["B"] | null | N<sub>2</sub>(g, 1 atom) $$\buildrel \, \over
\longrightarrow $$ N<sub>2</sub>(g, 5 atom)
<br><br>Here pressure increases. When pressure increases then the molecules of will come closer and intermoleculer distance decreases, so entropy will also decreases and $$\Delta S\, < \,0$$.
| mcq | jee-main-2018-online-16th-april-morning-slot | 4,145 |
nF98raqXNVt1Pqygegj2P | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | Given
<br/><br/>(i) 2Fe<sub>2</sub>O<sub>3</sub>(s) $$ \to $$ 4Fe(s) + 3O<sub>2</sub>(g);
<br/><br/>$$\Delta $$<sub>r</sub>G<sup>o</sup> = + 1487.0 kJ mol<sup>-1</sup>
<br/><br/>(ii) 2CO(g) + O<sub>2</sub>(g) $$ \to $$ 2CO<sub>2</sub>(g);
<br/><br/>$$\Delta $$<sub>r</sub>G<sup>o</sup> = $$-$$ 514.4 kJ mol<sup>-1<... | [{"identifier": "A", "content": "$$-$$ 112.4 kJ mol<sup>-1</sup>"}, {"identifier": "B", "content": "$$-$$ 56.2 kJ mol<sup>-1</sup>"}, {"identifier": "C", "content": "$$-$$ 168.2 kJ mol<sup>-1</sup>"}, {"identifier": "D", "content": "$$-$$ 208.0 kJ mol<sup>-1</sup>"}] | ["B"] | null | Given
<br><br>(i) 2Fe<sub>2</sub>O<sub>3</sub>(s) $$ \to $$ 4Fe(s) + 3O<sub>2</sub>(g);
<br><br>$$\Delta $$<sub>r</sub>G<sup>o</sup> = + 1487.0 kJ mol<sup>-1</sup>
<br><br>(ii) 2CO(g) + O<sub>2</sub>(g) $$ \to $$ 2CO<sub>2</sub>(g);
<br><br>$$\Delta $$<sub>r</sub>G<sup>o</sup> = $$-$$ 514.4 kJ... | mcq | jee-main-2018-online-15th-april-evening-slot | 4,146 |
7tRDrgv30LYuVdZQ9HiRw | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | $$\Delta $$<sub>f</sub>G<sup>o</sup> at 500 K for substance 'S' in liquid state and gaseous state are +100.7 kcl mol-<sup>1</sup> and +103 kcal mol<sup>-1</sup>, respectively. Vapour pressure of liquid 'S' at 500 K is approximately equal to : ( R = 2 cal K<sup>-1</sup> mol<sup>-1</sup> ) | [{"identifier": "A", "content": "0.1 atm"}, {"identifier": "B", "content": "1 atm"}, {"identifier": "C", "content": "10 atm"}, {"identifier": "D", "content": "100 atm"}] | ["A"] | null | S($$l$$) $$\buildrel \, \over
\longrightarrow $$ S(g)
<br><br>$$\Delta $$G<sup>o</sup> = $$\Delta $$<sub>f</sub>G<sup>o</sup> (Vapour) $$-$$ $$\Delta $$<sub>f</sub> G<sup>o</sup> (liquid)
<br><br>= 103 $$-$$ 100.7
<br><br>= 2.3 kcal / mol
<br><br>= 2.3 $$ \times $$ 10<sup>3</sup> cal/mol.
<br><... | mcq | jee-main-2018-online-15th-april-evening-slot | 4,147 |
N1hsjL3hpYi1Ssfw | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | Which of the following lines correctly show the temperature dependence of equilibrium constant K, for an
exothermic reaction?
<img src="data:image/png;base64,UklGRswNAABXRUJQVlA4IMANAABQVwCdASqXAQwBPm0yl0kkIqUhIjCZeKANiWlu4XJ+TRnZ1zfop/M/xz8E/6V+QHiH+d/tX5MZyT6p/Yv5//ZP9l/Uv3K/DP5d/p/4j5I++z4i9gL8p/h/9w/kn9P/z/9Z9Nf+u/... | [{"identifier": "A", "content": "A and D"}, {"identifier": "B", "content": "A and B"}, {"identifier": "C", "content": "B and C"}, {"identifier": "D", "content": "C and D"}] | ["B"] | null | We know from thermodynamics,
<br><br>$$\Delta $$G<sup>o</sup> = $$\Delta $$H<sup>o</sup> $$-$$ T$$\Delta $$S<sup>o</sup>
<br><br>$$ \Rightarrow \,\,\,\, - RT\ln K = \Delta {H^o} - T\Delta {S^o}$$
<br><br>$$ \Rightarrow \,\,\,\,\ln K = - {{\Delta {H^o}} \over R} \times {1 \over T} + {{\Delta {S^o}} \over R}.......\le... | mcq | jee-main-2018-offline | 4,148 |
qIUwi5Ml0Y7LZ3CDQH4tg | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | A process has $$\Delta $$H = 200 J mol<sup>–1</sup> and $$\Delta $$S = 40 JK<sup>–1</sup> mol<sup>–1</sup>. Out of the values given below, choose the minimum temperature above which the process will be spontaneous : | [{"identifier": "A", "content": "4 K"}, {"identifier": "B", "content": "20 K"}, {"identifier": "C", "content": "5 K"}, {"identifier": "D", "content": "12 K"}] | ["C"] | null | $$\Delta $$G = $$\Delta $$H $$-$$ T$$\Delta $$S
<br><br>T = $${{\Delta H} \over {\Delta S}} = {{200} \over {40}} = 5K$$ | mcq | jee-main-2019-online-10th-january-morning-slot | 4,149 |
qsZnQyDcywbXiTgy82w2w | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For the chemical reaction X $$\rightleftharpoons$$ Y, the standard reaction Gibbs energy depends on temperature T (in K) as
$$\Delta $$<sub>r</sub>G<sup>o</sup> (in kJ mol<sup>–1</sup>) = 120 $$ - {3 \over 8}$$ T.
<br/><br/>The major component of the reaction mixture at T is :
| [{"identifier": "A", "content": "Y if T = 300 K"}, {"identifier": "B", "content": "Y if T = 280 K "}, {"identifier": "C", "content": "X if T = 350 K"}, {"identifier": "D", "content": "X if T = 315 K "}] | ["D"] | null | X $$\rightleftharpoons$$ Y
<br><br>K<sub>eq</sub> = $${{\left[ Y \right]} \over {\left[ X \right]}}$$
<br><br>If K<sub>eq</sub> > 1 $$ \Rightarrow $$ [Y] > [X]
<br><br>and K<sub>eq</sub> < 1 $$ \Rightarrow $$ [Y] < [X]
<br><br>We know, $$\Delta $$G<sup>o</sup> = -RT ln(K<sub>eq</sub>)
<br><br>So when K<sub>... | mcq | jee-main-2019-online-11th-january-morning-slot | 4,150 |
vF0WDAdMB1lFuJfkX8Nux | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For the equilibrium,
<br/>2H<sub>2</sub>O $$\rightleftharpoons$$ H<sub>3</sub>O<sup>+</sup> + OH<sup>$$-$$</sup>, the value of $$\Delta $$G<sup>o</sup> at 298 K is approximately : | [{"identifier": "A", "content": "$$-$$ 80 kJ mol<sup>\u20131</sup>"}, {"identifier": "B", "content": "100 kJ mol<sup>$$-$$1</sup>"}, {"identifier": "C", "content": "$$-$$ 100 kJ mol<sup>$$-$$1</sup>"}, {"identifier": "D", "content": "80 kJ mol<sup>\u20131</sup>"}] | ["D"] | null | 2H<sub>2</sub>O $$\rightleftharpoons$$ H<sub>3</sub>O<sup>+</sup> + OH<sup>$$-$$</sup>
<br><br>Here K<sub>eq</sub> = K<sub>w</sub>(H<sub>2</sub>O)
<br><br>At 298 K, K<sub>w</sub>(H<sub>2</sub>O) = 10<sup>-14</sup>
<br><br>$$ \therefore $$ K<sub>eq</sub> = 10<sup>-14</sup>
<br><br>$$\Delta $$G<sup>o</sup> = -RTln(K<sub... | mcq | jee-main-2019-online-11th-january-evening-slot | 4,151 |
FNrh0oUQDHdLKsjYPZlmH | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The reaction, MgO(s) + C(s) $$ \to $$ Mg(s) + CO(g), for which $$\Delta $$<sub>r</sub>H<sup>o</sup> + 491.1 kJ mol<sup><sup>–1</sup></sup> and $$\Delta $$<sub>r</sub>S<sup>o</sup> = 198.0 JK<sup>–1</sup> mol<sup>–1</sup>, is not feasible at 298 K. Temperature above which reaciton will be feasible is :
| [{"identifier": "A", "content": "2480.3 K "}, {"identifier": "B", "content": "2040.5 K "}, {"identifier": "C", "content": "2380.5 K"}, {"identifier": "D", "content": "1890.0 K "}] | ["A"] | null | We know,
<br><br>$$\Delta $$G<sup>o</sup> = $$\Delta $$H<sup>o</sup> - T$$\Delta $$S<sup>o</sup>
<br><br>For a reaction to be spontaneous $$\Delta $$G<sup>o</sup> must be negative i.e.,
<br>T$$\Delta $$S<sup>o</sup> > $$\Delta $$H<sup>o</sup>
<br><br>$$ \Rightarrow $$ T > $${{\Delta H^\circ } \over {\Delta S^\cir... | mcq | jee-main-2019-online-11th-january-evening-slot | 4,152 |
yRVnKS7DGpKkm4pcsf3rsa0w2w9jwvd58pi | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | A process will be spontaneous at all temperatures if : | [{"identifier": "A", "content": "$$\\Delta $$H < 0 and $$\\Delta $$S > 0"}, {"identifier": "B", "content": "$$\\Delta $$H < 0 and $$\\Delta $$S < 0"}, {"identifier": "C", "content": "$$\\Delta $$H > 0 and $$\\Delta $$S < 0"}, {"identifier": "D", "content": "$$\\Delta $$H > 0 and $$\\Delta $$S > ... | ["A"] | null | A reaction is spontaneous if $$\Delta $$G is negative.
<br><br>and we know that
<br><br>$$\Delta $$G = $$\Delta $$H – T$$\Delta $$S
<br><br>If $$\Delta $$H = –ve and $$\Delta $$S = + ve then at all the temperature the process will be spontaneous.
| mcq | jee-main-2019-online-10th-april-morning-slot | 4,154 |
2xwG3K1hjILSUNpOO17k9k2k5e04gmb | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For the reaction :<br/><br/>
A($$l$$) $$ \to $$ 2B(g)<br/><br/>
$$\Delta U = 2.1\,kcal,\,\Delta S = 20\,cal\,{K^{ - 1}}$$ at 300 K<br/><br/>
Hence $$\Delta $$G in kcal is : | [] | null | -2.7 | A($$l$$) $$ \to $$ 2B(g)
<br><br>We know,
$$\Delta $$H = $$\Delta $$U + $$\Delta $$n<sub>g</sub>RT
<br><br>and $$\Delta $$G = $$\Delta $$H - T$$\Delta $$S
<br><br>$$ \therefore $$ $$\Delta $$G = $$\Delta $$U + $$\Delta $$n<sub>g</sub>RT - T$$\Delta $$S
<br><br>= 2.1 + $${{2 \times 2 \times 300} \over {1000}}$$ - $${{30... | integer | jee-main-2020-online-7th-january-morning-slot | 4,155 |
SKCkG6ju71QEK14WQEjgy2xukg3eriam | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For a reaction,
<br/>4M(s) + nO<sub>2</sub>(g) $$ \to $$ 2M<sub>2</sub>O<sub>n</sub>(s)
<br/>the free energy change is plotted as a function
of temperature. The temperature below which
the oxide is stable could be inferred from the
plot as the point at which : | [{"identifier": "A", "content": "the free energy change shows a change\nfrom negative to positive value"}, {"identifier": "B", "content": "the slope changes from positive to negative"}, {"identifier": "C", "content": "the slope changes from negative to positive"}, {"identifier": "D", "content": "the slope changes from ... | ["A"] | null | $$\Delta $$G = $$\Delta $$H – T$$\Delta $$S
<br><br>$$\Delta $$G = –ve (stable oxide)
<br><br>$$\Delta $$G = +ve (unstable oxide) | mcq | jee-main-2020-online-6th-september-evening-slot | 4,156 |
sUn1PiXlZzgbRtbfYm1klue4580 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For a chemical reaction A + B ⇌ C + D<br/><br/>($${\Delta _r}{H^\Theta }$$ = 80 kJ mol<sup>$$-$$1</sup>) the entropy change $${\Delta _r}{S^\Theta }$$ depends on the temperature T (in K) as $${\Delta _r}{S^\Theta }$$ = 2T (J K<sup>$$-$$1</sup>mol<sup>$$-$$1</sup>).<br/><br/>Minimum temperature at which it will become s... | [] | null | 200 | We know, $$\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ $$
<br><br>For a reaction to be spontaneous
<br>$$\Delta G^\circ < 0$$
<br><br>$$ \Rightarrow $$ $$\Delta H^\circ - T\Delta S^\circ < 0$$
<br><br>$$ \Rightarrow $$ $$T > {{\Delta H^\circ } \over {\Delta S^\circ }}$$
<br><br>$$ \Rightarrow $$ $$T... | integer | jee-main-2021-online-26th-february-morning-slot | 4,159 |
iUKFSnX9wqPPtSnJG21kmkinzyu | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | During which of the following processes, does entropy decrease?<br/><br/>(A) Freezing of water to ice at 0$$^\circ$$C<br/><br/>(B) Freezing of water to ice at $$-$$10$$^\circ$$C<br/><br/>(C) N<sub>2</sub>(g) + 3H<sub>2</sub>(g) $$ \to $$ 2NH<sub>3</sub>(g)<br/><br/>(D) Adsorption of CO(g) on lead surface.<br/><br/>(E) ... | [{"identifier": "A", "content": "(A), (C) and (E) only"}, {"identifier": "B", "content": "(B) and (C) only"}, {"identifier": "C", "content": "(A), (B), (C) and (D) only"}, {"identifier": "D", "content": "(A) and (E) only"}] | ["C"] | null | A, B $$ \to $$ Freezing of water will decrease entropy as particles will move closer and forces of
attraction will increase. This leads to decrease in randomness. So entropy decrease.<br><br>
C $$ \to $$ No. of molecules decreasing<br><br>
D $$ \to $$ Adsorption will lead to decrease in randomness of gaseous particles.... | mcq | jee-main-2021-online-17th-march-evening-shift | 4,160 |
1krrjiw4m | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For a given chemical reaction A $$\to$$ B at 300 K the free energy change is $$-$$49.4 kJ mol<sup>$$-$$1</sup> and the enthalpy of reaction is 51.4 kJ mol<sup>$$-$$1</sup>. The entropy change of the reaction is _____________ JK<sup>$$-$$1</sup> mol<sup>$$-$$1</sup>. | [] | null | 336 | $$\Delta$$G = $$-$$49.4 kJ/mol<br><br>$$\Delta$$H = 51.4 kJ/mol<br><br>$$\Delta$$G = $$\Delta$$H $$-$$ T$$\Delta$$S<br><br>$$-$$49400 = 51400 $$-$$ 300$$\Delta$$S<br><br>$$\Delta S = {{ + 100800} \over {300}} = 336$$ JK<sup>$$-$$1</sup> mol<sup>$$-$$1</sup> | integer | jee-main-2021-online-20th-july-evening-shift | 4,161 |
1ktfv68m5 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | Data given for the following reaction is as follows :<br/><br/>FeO<sub>(s)</sub> + C<sub>(graphite)</sub> $$\to$$ Fe<sub>(s)</sub> + CO<sub>(g)</sub><br/><br/><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-s... | [] | null | 964 | $${T_{\min }} = \left( {{{{\Delta ^0}H} \over {{\Delta ^0}S}}} \right)$$<br><br>$${\Delta ^0}{H_{rxn}} = \left[ {\Delta _f^0H(Fe) + \Delta _f^0H(CO)} \right] - $$<br><br>$$ = \left[ {\Delta _f^0H(FeO) + \Delta _f^0H({C_{(graphite)}})} \right]$$<br><br>$$ = [0 - 110.5] - [ - 266.3 + 0]$$<br><br>= 155.8 kJ/mol<br><br>$${... | integer | jee-main-2021-online-27th-august-evening-shift | 4,162 |
1ktjvsvso | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | The incorrect expression among the following is : | [{"identifier": "A", "content": "$${{\\Delta {G_{System}}} \\over {\\Delta {S_{Total}}}} = - T$$ (at constant P)"}, {"identifier": "B", "content": "$$K = {{\\Delta H^\\circ - T\\Delta S^\\circ } \\over {RT}}$$"}, {"identifier": "C", "content": "$$K = {e^{ - \\Delta G^\\circ /RT}}$$"}, {"identifier": "D", "content": "... | ["B"] | null | Option (b) is incorrect.<br><br>$$\Delta$$G$$^\circ$$ = $$-$$RT ln K<br><br>$$\Delta$$H$$^\circ$$ $$-$$ T$$\Delta$$S$$^\circ$$ = $$-$$RT ln K<br><br>ln K = $$\left[ {{{\Delta H^\circ - \Delta S^\circ } \over {RT}}} \right]$$ | mcq | jee-main-2021-online-31st-august-evening-shift | 4,163 |
1l5ami5uk | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>The standard entropy change for the reaction</p>
<p>4Fe(s) + 3O<sub>2</sub>(g) $$\to$$ 2Fe<sub>2</sub>O<sub>3</sub>(s) is $$-$$550 J K<sup>$$-$$1</sup> at 298 K.</p>
<p>[Given : The standard enthalpy change for the reaction is $$-$$165 kJ mol<sup>$$-$$1</sup>]. The temperature in K at which the reaction attains equ... | [] | null | 300 | $\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}=0$ at equilibrium<br/><br/>
$$
\begin{aligned}
&\Rightarrow-165 \times 10^3-\mathrm{T} \times(-505)=0 \\\\
&\Rightarrow \mathrm{T}=300 \mathrm{~K}
\end{aligned}
$$ | integer | jee-main-2022-online-25th-june-morning-shift | 4,165 |
1l6nunztx | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>Given below are two statements: One is labelled as Assertion $$\mathbf{A}$$ and the other is labelled as Reason $$\mathbf{R}$$</p>
<p>Assertion A : The reduction of a metal oxide is easier if the metal formed is in liquid state than solid state.</p>
<p>Reason $$\mathbf{R}$$ : The value of $$\Delta G ^\Theta$$ become... | [{"identifier": "A", "content": "Both A and R are correct and R is the correct explanation of A"}, {"identifier": "B", "content": "Both A and R are correct but R is NOT the correct explanation of A"}, {"identifier": "C", "content": "A is correct but R is not correct"}, {"identifier": "D", "content": "A is not correct b... | ["A"] | null | Reduction of a metal oxide is easier if the metal is formed in a liquid state at the temperature of reduction because the entropy is higher if the metal is in a liquid state. | mcq | jee-main-2022-online-28th-july-evening-shift | 4,167 |
1ldyh7zou | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>For independent process at 300 K</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:s... | [] | null | 2 | $$
\begin{aligned}
& \Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S} \\\\
& \mathrm{A}: \Delta \mathrm{G}\left(\mathrm{J} \mathrm{mol}^{-1}\right)=-25 \times 10^3+80 \times 300:-\mathrm{ve} \\\\
& \mathrm{B}: \Delta \mathrm{G}\left(\mathrm{J} \mathrm{mol}^{-1}\right)=-22 \times 10^3-40 \times 300:-\mat... | integer | jee-main-2023-online-24th-january-morning-shift | 4,168 |
lgo0frci | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | $30.4 \mathrm{~kJ}$ of heat is required to melt one mole of sodium chloride and the entropy change at the melting point is $28.4 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ at 1 atm. The melting point of sodium chloride is _______________ K (Nearest Integer) | [] | null | 1070 | The heat required to melt one mole of a substance is known as its molar enthalpy of fusion, denoted as $\Delta H_\mathrm{fus}$. For sodium chloride, $\Delta H_\mathrm{fus}$ is $30.4\ \mathrm{kJ/mol}$.
<br/><br/>
The entropy change at the melting point is given by $\Delta S = \frac{\Delta H_\mathrm{fus}}{T_\mathrm{m}}$... | integer | jee-main-2023-online-15th-april-morning-shift | 4,169 |
1lgyt32qk | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>For complete combustion of ethene.</p>
<p>$$\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})+3 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$$</p>
<p>the amount of heat produced as measured in bomb calorimeter is $$1406 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ at $$30... | [] | null | 1411 | <p>In the given combustion reaction, the number of moles of gaseous products ($\Delta n_g$) is -2 (since we have 2 moles of CO₂ gas on the product side and 4 moles of gaseous reactants). </p>
<p>The change in internal energy ($\Delta U$) is given as -1406 kJ/mol.<br/><br/> We can calculate the change in enthalpy ($\Del... | integer | jee-main-2023-online-8th-april-evening-shift | 4,170 |
1lh29rrt0 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>The value of $$\log \mathrm{K}$$ for the reaction $$\mathrm{A} \rightleftharpoons \mathrm{B}$$ at $$298 \mathrm{~K}$$ is ___________. (Nearest integer)</p>
<p>Given: $$\Delta \mathrm{H}^{\circ}=-54.07 \mathrm{~kJ} \mathrm{~mol}^{-1}$$</p>
<p>$$\Delta \mathrm{S}^{\circ}=10 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{... | [] | null | 10 | <p>Given:<br/><br/>
$$
\begin{align}
\Delta H^0 & = -54.07 \, \text{kJ/mol} = -54070 \, \text{J/mol} \\\\
\Delta S^0 & = 10 \, \text{J/K}\cdot \text{mol} \\\\
T & = 298 \, \text{K}
\end{align}
$$</p>
<p>We find the change in Gibbs free energy $\Delta G^0$:<br/><br/>
$$
\begin{align}
\Delta G^0 & = \Delt... | integer | jee-main-2023-online-6th-april-morning-shift | 4,172 |
lsapb10m | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | For a certain reaction at $300 \mathrm{~K}, \mathrm{~K}=10$, then $\Delta \mathrm{G}^{\circ}$ for the same reaction is - ____________ $\times 10^{-1} \mathrm{~kJ} \mathrm{~mol}^{-1}$.<br/><br/> (Given $\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ ) | [] | null | 57 | <p>To determine the change in standard Gibbs free energy ($\Delta G^{\circ}$) for the reaction at a given temperature when the equilibrium constant ($K$) is known, we can use the following relationship:</p>
<p>$$ \Delta G^{\circ} = -RT \ln K $$
</p>
<p>Here, $R$ is the universal gas constant ($8.314 \ J K^{-1} mol^{-1... | integer | jee-main-2024-online-1st-february-evening-shift | 4,173 |
jaoe38c1lse8bprp | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>Consider the following reaction at $$298 \mathrm{~K} \cdot \frac{3}{2} \mathrm{O}_{2(g)} \rightleftharpoons \mathrm{O}_{3(g)} \cdot \mathrm{K}_{\mathrm{P}}=2.47 \times 10^{-29}$$. $$\Delta_r G^{\ominus}$$ for the reaction is _________ $$\mathrm{kJ}$$. (Given $$\mathrm{R}=8.314 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}$$)... | [] | null | 163 | <p>$$\begin{aligned}
& \frac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{O}_{3(\mathrm{~g})} \cdot \mathrm{K}_{\mathrm{P}}=2.47 \times 10^{-29} . \\
& \Delta_{\mathrm{r}} \mathrm{G}^{\Theta}=-\mathrm{RT} \ln \mathrm{K}_{\mathrm{P}} \\
& =-8.314 \times 10^{-3} \times 298 \times \ln \left(2.47 \times 10^... | integer | jee-main-2024-online-31st-january-morning-shift | 4,175 |
jaoe38c1lsfjpymm | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>Which of the following is not correct?</p> | [{"identifier": "A", "content": "$$\\Delta \\mathrm{G}$$ is positive for a spontaneous reaction\n"}, {"identifier": "B", "content": "$$\\Delta \\mathrm{G}$$ is positive for a non-spontaneous reaction\n"}, {"identifier": "C", "content": "$$\\Delta \\mathrm{G}$$ is zero for a reversible reaction\n"}, {"identifier": "D", ... | ["A"] | null | <p>The statement that is not correct among the given options is Option A.</p>
<p>Option A states that $$\Delta \mathrm{G}$$ is positive for a spontaneous reaction, which is incorrect. The criterion for spontaneity in a chemical reaction is based on the Gibbs free energy change ($$\Delta \mathrm{G}$$) for the process. ... | mcq | jee-main-2024-online-29th-january-morning-shift | 4,176 |
luy1mwsk | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>When $$\Delta \mathrm{H}_{\mathrm{vap}}=30 \mathrm{~kJ} / \mathrm{mol}$$ and $$\Delta \mathrm{S}_{\mathrm{vap}}=75 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$$, then the temperature of vapour, at one atmosphere is _________ K.</p> | [] | null | 400 | <p>To find the temperature of vaporization at one atmosphere, we can use the Clausius-Clapeyron equation, which relates the enthalpy of vaporization ($$\Delta H_{vap}$$) to the change in entropy ($$\Delta S_{vap}$$) during the phase transition at a particular temperature (T). The relationship can be simplified under th... | integer | jee-main-2024-online-9th-april-evening-shift | 4,177 |
lvb2a8u8 | chemistry | thermodynamics | entropy,-free-energy-change-and-spontaneity | <p>For the reaction at $$298 \mathrm{~K}, 2 \mathrm{~A}+\mathrm{B} \rightarrow \mathrm{C}, \Delta \mathrm{H}=400 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ and $$\Delta S=0.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$$. The reaction will become spontaneous above __________ $$\mathrm{K}$$.</p> | [] | null | 2000 | <p>To determine the temperature above which the reaction $$2A+B \rightarrow C$$ becomes spontaneous, we can use the Gibbs free energy equation:</p>
<p>$$\Delta G = \Delta H - T\Delta S$$</p>
<p>The reaction becomes spontaneous when $$\Delta G$$ is negative. Therefore, we need to find the temperature at which $$\Delta... | integer | jee-main-2024-online-6th-april-evening-shift | 4,178 |
98FjQESVhnjwpe5h | chemistry | thermodynamics | first-law-of-thermodynamics | A heat engine absorbs heat Q<sub>1</sub> at temperature T<sub>1</sub> and heat Q<sub>2</sub> at temperature T<sub>2</sub>. Work done by the engine is J (Q<sub>1</sub> + Q<sub>2</sub>). This data : | [{"identifier": "A", "content": "violates 1<sup>st</sup> law of thermodynamics"}, {"identifier": "B", "content": "violates 1<sup>st</sup> law of thermodynamics if Q<sub>1</sub> is +ve"}, {"identifier": "C", "content": "violates 1<sup>st</sup> law of thermodynamics if Q<sub>1</sub> is -ve"}, {"identifier": "D", "content... | ["A"] | null | According to first law of thermodynamics energy can neither be created nor destroyed although it can be converted from one form to another.
<br><br><b>NOTE :</b> Carnot cycle is based upon this principle but during the conversion of heat into work some mechanical energy is always converted to other form of energy henc... | mcq | aieee-2002 | 4,179 |
CtnAEjRAXdaaaS5f | chemistry | thermodynamics | first-law-of-thermodynamics | The internal energy change when a system goes from state A to B is 40 kJ/mole. If the system goes from A to B by a reversible path and returns to state A by an irreversible path what would be the net change in internal energy? | [{"identifier": "A", "content": "> 40 kJ"}, {"identifier": "B", "content": "< 40 kJ"}, {"identifier": "C", "content": "Zero"}, {"identifier": "D", "content": "40 kJ"}] | ["C"] | null | For a cyclic process the net change in the internal energy is zero because the change in internal energy does not depend on the path.
<br><br><img class="question-image" src="https://res.cloudinary.com/dckxllbjy/image/upload/v1734265867/exam_images/kdnkykcecyti11syp5sf.webp" loading="lazy" alt="AIEEE 2003 Chemistry - T... | mcq | aieee-2003 | 4,180 |
5pH25xJQ6F1NJ5Kz | chemistry | thermodynamics | first-law-of-thermodynamics | A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant
temperature of 37.0<sup>o</sup>C. As it does so, it absorbs 208J of heat. The values of q and w for the process will be :<br/>
(R = 8.314 J/mol K) ( l n 7.5 = 2.01) | [{"identifier": "A", "content": "q = \u2013 208 J, w = \u2013 208 J "}, {"identifier": "B", "content": "q = \u2013 208 J, w = + 208 J"}, {"identifier": "C", "content": "q = + 208 J, w = + 208 J"}, {"identifier": "D", "content": "q = + 208 J, w = \u2013 208 J "}] | ["D"] | null | By I<sup>st</sup>
law of thermodynamics, q = $$\Delta $$E – W
<br><br>At const T, ∆E = 0
<br><br> q = – W
<br><br> Heat absorbed = 208 J
<br><br>$$ \therefore $$ q = +208 J
<br><br> W = – 208 J | mcq | jee-main-2013-offline | 4,183 |
FLF00zYKOUeO5QsyAig0F | chemistry | thermodynamics | first-law-of-thermodynamics | If 100 mole of H<sub>2</sub>O<sub>2</sub> decompose at 1 bar and 300 K, the work done (kJ) by one mole of O<sub>2</sub>(g) as it expands against 1 bar pressure is :
<br/><br/>2H<sub>2</sub>O<sub>2</sub>(l) $$\rightleftharpoons$$ 2H<sub>2</sub>O(l) + O<sub>2</sub>(g)
<br/><br/>(R = 8.3 J K <sup>$$-$$1</sup> mol<s... | [{"identifier": "A", "content": "62.25"}, {"identifier": "B", "content": "124.50"}, {"identifier": "C", "content": "249.00"}, {"identifier": "D", "content": "498.00"}] | ["C"] | null | <p>For reaction : 2H<sub>2</sub>O<sub>2</sub>(1) $$\rightleftharpoons$$ 2H<sub>2</sub>O(1) + O<sub>2</sub>(g)</p>
<p>Given, p = 1 bar, T = 300 K, n = 100 mol, R = 8.3 J K<sup>$$-$$</sup> mol<sup>$$-$$1</sup></p>
<p>We know that</p>
<p>w = p$$\Delta$$V = nRT</p>
<p>= 100 $$\times$$ 8.3 $$\times$$ 300</p>
<p>= 249000 J o... | mcq | jee-main-2016-online-10th-april-morning-slot | 4,184 |
jsgorkZ6BUuFnGFy | chemistry | thermodynamics | first-law-of-thermodynamics | $$\Delta $$U is equal to : | [{"identifier": "A", "content": "Isobaric work"}, {"identifier": "B", "content": "Adiabatic work "}, {"identifier": "C", "content": "Isothermal work "}, {"identifier": "D", "content": "Isochoric work "}] | ["B"] | null | From 1st law of thermodynamics
<br><br>ΔU = q + w
<br><br>For adiabatic process :
<br><br>q = 0
<br><br>$$ \therefore $$ ΔU = w
<br><br>So change in internal energy (ΔU) is equal to adiabatic work. | mcq | jee-main-2017-offline | 4,185 |
g9p0EYnRxA9Rv09nJWZHu | chemistry | thermodynamics | first-law-of-thermodynamics | A gas undergoes change from state A to state B. In this process, the heat absorbed
and work done by the gas is 5 J and 8 J, respectively. Now gas is brought back to
A by another process during which 3 J of heat is evolved. In this reverse process of
B to A : | [{"identifier": "A", "content": "10 J of the work will be done by the gas. "}, {"identifier": "B", "content": "6 J of the work will be done by the gas."}, {"identifier": "C", "content": "10 J of the work will be done by the surrounding on gas.\n"}, {"identifier": "D", "content": "6 J of the work will be done by the sur... | ["D"] | null | <p>From first law of thermodynamics, we have</p>
<p>$$\Delta$$U = q + w</p>
<p>$$\bullet$$ For state A to B : q = +5 J, w = $$-$$8 J and</p>
<p>$$\Delta$$U<sub>AB</sub> = 5 + ($$-$$8) = $$-$$3 J</p>
<p>$$\bullet$$ For state B to A : q = $$-$$3 J</p>
<p>Since the internal energy is a state function, we have $$\Delta$$U<... | mcq | jee-main-2017-online-9th-april-morning-slot | 4,186 |
KscWeSbFVgtMMb6MKUO8d | chemistry | thermodynamics | first-law-of-thermodynamics | An ideal gas undergoes a cyclic process as shown in Figure.
<br/><br/><img src="data:image/png;base64,UklGRuQLAABXRUJQVlA4INgLAAAw/QCdASoAA/gCP4HA32U2Ma+nIdb4+sAwCWlu4XPTqmNwvjSDe8qh7mYjz1QfX/uZnf4YKSGCpNbHR5r4bbo818Nt0ea+G26PNfDbcbxXBzDqArptE9A6HcNt0ea+G26PNfDbdHmvhtqE3NyzDZCRGoFftVkwBxwkBpae7EOpVvdiHUq3uxDqUGcdhx6G7c... | [{"identifier": "A", "content": "$$-$$5 kJ mol<sup>-1</sup>"}, {"identifier": "B", "content": "+5 kJ mol<sup>-1</sup>"}, {"identifier": "C", "content": "18 kJ mol<sup>-1</sup>"}, {"identifier": "D", "content": "$$-$$18 kJ mol<sup>-1</sup>"}] | ["B"] | null | Given,
<br><br>$$\Delta $$U<sub>BC</sub> = $$-$$ 5 kJ/mol
<br><br>$$\Delta $$U<sub>AB</sub> = q<sub>AB</sub> + W<sub>AB</sub>
<br><br>= 2 + ($$-$$ 5)
<br><br>= $$-$$ 3 kJ/mol.
<br><br>For cyclic process,
<br><br>$$\Delta $$U = 0
<br><br>$$ \Rightarrow $$$$\,\,\,\,$$ $$\Delta $$U<sub>AB</sub> + $$\Delta $$U<sub>BC</sub... | mcq | jee-main-2018-online-15th-april-morning-slot | 4,187 |
u2tCpn0kWEsKdZBzxVhRC | chemistry | thermodynamics | first-law-of-thermodynamics | 5 moles of an ideal gas at 100 K are allowed
to undergo reversible compression till its
temperature becomes 200 K.
If C<sub>V</sub> = 28 JK<sup>–1</sup>mol<sup>–1</sup>, calculate $$\Delta $$U and $$\Delta $$pV for
this process. (R = 8.0 JK<sup>–1</sup> mol<sup>–1</sup>] | [{"identifier": "A", "content": "$$\\Delta $$U = 14 kJ; $$\\Delta $$(pV) = 4 kJ"}, {"identifier": "B", "content": "$$\\Delta $$U = 2.8 kJ; $$\\Delta $$(pV) = 0.8 kJ"}, {"identifier": "C", "content": "$$\\Delta $$U = 14 kJ; $$\\Delta $$(pV) = 18 kJ"}, {"identifier": "D", "content": "$$\\Delta $$U = 14 kJ; $$\\Delta $$(p... | ["A"] | null | For ideal gas,
<br><br>$$\Delta $$U = nC<sub>v</sub>$$\Delta $$T
<br><br>= 5 $$ \times $$ 28 $$ \times $$ (200 - 100)
<br><br>= 14 kJ
<br><br>We know,
<br><br>PV = nRT
<br><br>$$ \therefore $$ $$\Delta $$(PV) = nR$$\Delta $$T = 5 $$ \times $$ 8 $$ \times $$ 100 = 4 kJ | mcq | jee-main-2019-online-8th-april-evening-slot | 4,188 |
uZvgJnxKsRyuimysh3fCg | chemistry | thermodynamics | first-law-of-thermodynamics | An ideal gas undergoes isothermal compression from 5m<sup>3</sup> to 1 m<sup>3</sup> against a constant external pressure of 4 Nm<sup>–2</sup>. Heat released in this process is used to increase the temperature of 1 mole of Al. If molar heat capacity of Al is 24 J mol<sup>–1</sup> K<sup>–1</sup>, the temperature of Al ... | [{"identifier": "A", "content": "$${2 \\over 3}K$$"}, {"identifier": "B", "content": "$${3 \\over 2}K$$"}, {"identifier": "C", "content": "1 K"}, {"identifier": "D", "content": "2 K"}] | ["A"] | null | Work done on isothermal irreversible for ideal gas
<br><br>= $$-$$P<sub>ext</sub> (V<sub>2</sub> $$-$$ V<sub>1</sub>)
<br><br>= $$-$$4 N/m<sup>2</sup> (1 m<sup>3</sup> $$-$$ 5m<sup>3</sup>)
<br><br>= 16 Nm
<br><br>Isothermal process for ideal gas
<br><br>$$\Delta $$U = 0
<br><br>q = $$-$$ w
<br><br>= $$-$$ 16 Nm
<br... | mcq | jee-main-2019-online-10th-january-evening-slot | 4,192 |
IETnnCsV7Kq9Kde7Gu7k9k2k5h77ko1 | chemistry | thermodynamics | first-law-of-thermodynamics | The magnitude of work done by a gas that undergoes a reversible expansion along the path ABC shown in
the figure is _______.
<img src="data:image/png;base64,UklGRtQSAABXRUJQVlA4IMgSAAAQcwCdASrlATABPm02mEikIqKhIrJZgIANiWlu4XShG/OT8S/xr8gvBn+0/2D9p/Eh8x/Z/yr/pvr8Vg/8r/K/NX9d/vv8l/qP/F/v3zp/O/71/Nf2Y84fb1/R+oX6n/uv80/r3/U... | [] | null | 48 | Work done = Area covered by the diagram
<br/><br/>= $$1\over2$$ × (sum of parallel sides) × height
<br/><br/>= $$1\over2$$ × (10+6) × 6<br/><br/>
= $$1\over2$$ × 16 × 6
<br/><br/> = 48 Joule
<br><br><b>Note :</b> Here pressure difference = 8 - 2 = 6 Pa and volume difference = 12 - 2 = 10 | integer | jee-main-2020-online-8th-january-morning-slot | 4,193 |
agnOphGtqdEAlBmEV0jgy2xukfcepdd9 | chemistry | thermodynamics | first-law-of-thermodynamics | Five moles of an ideal gas at 1 bar and 298 K
is expanded into vacuum to double the volume.
The work done is : | [{"identifier": "A", "content": "Zero"}, {"identifier": "B", "content": "-RT $$\\ln {{{V_2}} \\over {{V_1}}}$$"}, {"identifier": "C", "content": "C<sub>V</sub> (T<sub>2</sub> \u2013 T<sub>1</sub>)"}, {"identifier": "D", "content": "\u2013 RT (V<sub>2</sub> \u2013 V<sub>1</sub>)"}] | ["A"] | null | As the expansion is done in vacuum that is in absence <br>of p<sub>ext</sub> so
p<sub>ext</sub> = 0
<br><br>$$ \therefore $$ W = - p<sub>ext</sub>$$\Delta $$V
<br><br>= 0 | mcq | jee-main-2020-online-4th-september-evening-slot | 4,195 |
5sHGvFiuF0dKLYUk1A1klsc02di | chemistry | thermodynamics | first-law-of-thermodynamics | The reaction of cyanamide, NH<sub>2</sub>CN<sub>(s)</sub> with oxygen was run in a bomb calorimeter and $$\Delta$$U was found to be $$-$$742.24 kJ mol<sup>$$-$$1</sup>. The magnitude of $$\Delta$$H<sub>298</sub> for the reaction<br/><br/>$$N{H_2}C{H_{(S)}} + {3 \over 2}{O_{2(g)}} \to {N_{2(g)}} + {O_{2(g)}} + {H_2}{O_{... | [] | null | 741 | $$N{H_2}CN(s) + {3 \over 2}{O_2}(g)\buildrel {} \over
\longrightarrow {N_2}(g) + C{O_2}(g) + {H_2}O(l)$$<br><br>$$\Delta ng = (1 + 1) - {3 \over 2} = {1 \over 2}$$<br><br>$$\Delta H = \Delta U + \Delta ng\,RT$$<br><br>$$ = - 742.24 + {1 \over 2} \times {{8.314 \times 298} \over {1000}}$$<br><br>$$ = - 742.24 + 1.24$... | integer | jee-main-2021-online-25th-february-morning-slot | 4,196 |
VTSpv3S8oolZSwsX081kmiuvlog | chemistry | thermodynamics | first-law-of-thermodynamics | At 25$$^\circ$$C, 50 g of iron reacts with HCl to form FeCl<sub>2</sub>. The evolved hydrogen gas expands against a constant pressure of 1 bar. The work done by the gas during this expansion is _________ J. (Round off to the Nearest Integer).<br/><br/>[Given : R = 8.314 J mol<sup>$$-$$1</sup> K<sup>$$-$$1</sup>. Assume... | [] | null | 2218 | $$Fe + 2HCl \to FeC{l_2} + {H_2}$$<br><br>$${{50} \over {55.85}}moles$$
<br><br>Moles of Fe = $${{50} \over {55.85}}moles$$ = Moles of H<sub>2</sub>
<br><br>No. of H<sub>2</sub> produced $$ = {{50} \over {55.85}}moles$$<br><br>Work done $$ = - {P_{ext}}\,.\,\Delta V$$<br><br>$$ = - \Delta {n_g}RT$$<br><br>$$ = - {{5... | integer | jee-main-2021-online-16th-march-evening-shift | 4,198 |
1krxbdi4f | chemistry | thermodynamics | first-law-of-thermodynamics | A system does 200 J of work and at the same time absorbs 150 J of heat. The magnitude of the change in internal energy is ____________ J. (Nearest integer) | [] | null | 50 | w = $$-$$200 J, q = +150 : $$\Delta$$U = q + w<br><br>$$\Delta$$U = 150 $$-$$ 200 = $$-$$50 J <br><br>Magnitude = 50 J = |$$\Delta$$U | | integer | jee-main-2021-online-25th-july-evening-shift | 4,199 |
1l54z4o3a | chemistry | thermodynamics | first-law-of-thermodynamics | <p>2.2 g of nitrous oxide (N<sub>2</sub>O) gas is cooled at a constant pressure of 1 atm from 310 K to 270 K causing the compression of the gas from 217.1 mL to 167.75 mL. The change in internal energy of the process, $$\Delta$$U is '$$-$$x' J. The value of 'x' is ________. [nearest integer]</p>
<p>(Given : atomic mass... | [] | null | 195 | $\Delta T=-40 \mathrm{~K}$
<br/><br/>
$$
\begin{aligned}
\Delta U &=q+w \\\\
&=\frac{100 \times 2.2}{44}(-40)-(-49.39) \times 10^{-3} \times 101.325
\end{aligned}
$$
<br/><br/>
$$
\begin{aligned}
&=-200+5 \\\\
&=-195 \mathrm{~J} \\\\
\mathrm{x}=& 195
\end{aligned}
$$ | integer | jee-main-2022-online-29th-june-evening-shift | 4,200 |
1l56bgaqs | chemistry | thermodynamics | first-law-of-thermodynamics | <p>4.0 L of an ideal gas is allowed to expand isothermally into vacuum until the total volume is 2.0 L. The amount of heat absorbed in this expansion is ____________ L atm.</p> | [] | null | 0 | Work done $=-P_{\text {ext }} \Delta \mathrm{v}$
<br/><br/>
$$
\because P_{\text {ext }}=0 \quad \text { (vacuum) }
$$
<br/><br/>
$\therefore w=0, \quad\Delta U=0$ (as the process is isothermal)
<br/><br/>
So, $q=0$ | integer | jee-main-2022-online-28th-june-morning-shift | 4,201 |
1l58k60op | chemistry | thermodynamics | first-law-of-thermodynamics | <p>A fish swimming in water body when taken out from the water body is covered with a film of water of weight 36 g. When it is subjected to cooking at 100$$^\circ$$C, then the internal energy for vaporization in kJ mol<sup>$$-$$1</sup> is ___________. [nearest integer]</p>
<p>[Assume steam to be an ideal gas. Given $$\... | [] | null | 38 | $\underset{36 \mathrm{~g}}{\mathrm{H}_{2} \mathrm{O}}(\ell) \longrightarrow \underset{36 \mathrm{~g}}{\mathrm{H}_{2} \mathrm{O}}(\mathrm{g})$ (evaporation)
<br/><br/>
$$
\begin{aligned}
\mathrm{n}_{\mathrm{H}_{2} \mathrm{O}} &=\frac{36}{18}=2 \quad \Delta \mathrm{n}_{\mathrm{g}}=1-0=1 \\\\
\Delta \mathrm{U}_{\text {vap... | integer | jee-main-2022-online-26th-june-evening-shift | 4,202 |
1l6jmyzvl | chemistry | thermodynamics | first-law-of-thermodynamics | <p>The molar heat capacity for an ideal gas at constant pressure is $$20.785 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$$. The change in internal energy is $$5000 \mathrm{~J}$$ upon heating it from $$300 \mathrm{~K}$$ to $$500 \mathrm{~K}$$. The number of moles of the gas at constant volume is ____________. [Neare... | [] | null | 2 | $\mathrm{C}_{\mathrm{p}}=20.785 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$
<br/><br/>
$$
\begin{aligned}
&\text { and } \Delta \mathrm{U}=\mathrm{nC} \mathrm{v} \Delta \mathrm{T} \\\\
&\therefore \quad \mathrm{nC}_{\mathrm{v}}=\frac{5000}{200}=25
\end{aligned}
$$
<br/><br/>
and we know that
<br/><br/>
$$
\begin{... | integer | jee-main-2022-online-27th-july-morning-shift | 4,203 |
1l6kuhdow | chemistry | thermodynamics | first-law-of-thermodynamics | <p>A gas (Molar mass = 280 $$\mathrm{~g} \mathrm{~mol}^{-1}$$) was burnt in excess $$\mathrm{O}_{2}$$ in a constant volume calorimeter and during combustion the temperature of calorimeter increased from $$298.0 \mathrm{~K}$$ to $$298.45$$ $$\mathrm{K}$$. If the heat capacity of calorimeter is $$2.5 \mathrm{~kJ} \mathrm... | [] | null | 35 | $\Delta \mathrm{U}=\mathrm{C} \Delta \mathrm{T}$
<br/><br/>
$$
\begin{aligned}
&=2.5 \times 10^{3} \times 0.45 \\\\
&=1.125 \mathrm{~kJ}
\end{aligned}
$$
<br/><br/>
Considering $\Delta \mathrm{H} \simeq \Delta \mathrm{U}$
<br/><br/>
$$
\Delta \mathrm{H}=9 \mathrm{~kJ} / \mathrm{mol} \simeq \Delta \mathrm{U}
$$
<br/><br... | integer | jee-main-2022-online-27th-july-evening-shift | 4,204 |
ldqy1ec0 | chemistry | thermodynamics | first-law-of-thermodynamics | 1 mole of ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27^{\circ} \mathrm{C}$. The work done is $3 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The final temperature of the gas is ________ $\mathrm{K}$ (Nearest integer).<br/><br/> Given $\mathrm{C_V}=20 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{... | [] | null | 150 | <p>$$\mathrm{T_1=300~K}$$</p>
<p>$$\mathrm{w = 3}$$ kJ/mole</p>
<p>$$\mathrm{w=nC_v\Delta T}$$</p>
<p>$$3000=1\times20\times(300-\mathrm{T_2})$$</p>
<p>$$300-\mathrm{T_2}=150$$</p>
<p>$$\mathrm{T_2=150~K}$$</p> | integer | jee-main-2023-online-30th-january-evening-shift | 4,205 |
1ldr52d12 | chemistry | thermodynamics | first-law-of-thermodynamics | <p>When 2 litre of ideal gas expands isothermally into vacuum to a total volume of 6 litre, the change in internal energy is ____________ J. (Nearest integer)</p> | [] | null | 0 | <p>For isothermal process of an ideal gas; $$\mathrm{\Delta E=0}$$</p> | integer | jee-main-2023-online-30th-january-morning-shift | 4,206 |
1ldulzecp | chemistry | thermodynamics | first-law-of-thermodynamics | <p>An athlete is given 100 g of glucose (C$$_6$$H$$_{12}$$O$$_6$$) for energy. This is equivalent to 1800kJ of energy. The 50% of this energy gained is utilized by the athlete for sports activities at the event. In order to avoid storage of energy, the weight of extra water he would need to perspire is ____________ g (... | [] | null | 360 | $$
\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6(\mathrm{~s})+6 \mathrm{O}_2 \rightarrow 6 \mathrm{CO}_2(\mathrm{~g})+6 \mathrm{H}_2 \mathrm{O}(\mathrm{l})
$$<br/><br/>
Extra energy used to convert $\mathrm{H}_2 \mathrm{O(l)}$ into $\mathrm{H}_2 \mathrm{O}(\mathrm{l})$ into $\mathrm{H}_2 \mathrm{O}(\mathrm{g})$<br/><br/>
$... | integer | jee-main-2023-online-25th-january-morning-shift | 4,207 |
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