instruction stringlengths 15 21.8k |
|---|
In my textbook, it's written that vapour pressure of a liquid does not depend on shape and size of a container but won't a container that provides less surface area to the liquid will have lower vapour pressure?
for example, consider 2 containers give in the diagram below, the volume of container and liquid is same ... |
Why is vapour pressure not dependent on shape and size of the container? |
What is the right way to calculate concentration of volatile compounds in the air in close container?
Let's assume we have a 50ml bottle with 25ml of 100% Ethanol in it.
Will it be right to use the PV=nRT equation in that case?
So in that cause it will be
P(ethanol) = 0.05872 atm;
V = 0.025 L;
R = 0.08206... |
What is the right way to calculate the concentration of volatile compounds in the air in a closed container?
Suppose we have a $50\ mL$ bottle with $25\ mL$ of $100\ %$ ethanol (EtOH) in it.
In this case, will it be okay to use $PV=nRT$ ?
Doing so, it will be:
$$P_{EtOH} = 0.05872\ atm$$
$$V = 0.025\ L$$
... |
What is the right way to calculate the concentration of volatile compounds in the air in a closed container?
Suppose we have a $50\ mL$ bottle with $25\ mL$ of $100\ %$ ethanol (EtOH) in it.
In this case, will it be okay to use $PV=nRT$ ?
Doing so, it will be:
$$P_{EtOH} = 0.05872\ atm$$
$$V = 0.025\ L$$
... |
Yes, you're exactly right. Not only is the axial methyl gauche with respect to the methylene unit that you point out, but there are also gauche interactions of the two methylenes that are drawn in the "bridging" positions of your Newman projections.
So, why is the chair conformation so stable?
For one, gauche int... |
What is the right way to calculate the concentration of volatile compounds in the air in a closed container?
Suppose we have a $50\ mL$ bottle with $25\ mL$ of $100\ %$ ethanol (EtOH) in it.
In this case, will it be okay to use $PV=nRT$ ?
Doing so, it will be:
$$P_{EtOH} = 0.05872\ atm$$
$$V = 0.025\ L$$
... |
How would you guys interpret the IR spectrum of your product if it's peaks match the literature spectrum, but the signals are weak? Could saying that the sample was very dilute and there was lots of water work as a viable explanation?
What about in a scenario where the experimental IR spectrum has all necessary peak... |
Intensity is (in general) proportional to sample concentration, so yes, if you are performing IR in solution, then an overly dilute sample would have less intense peaks. But solution IR is somewhat uncommon; I suspect you are either doing IR on your sample in neat form (using an ATR stage) or in a pressed KBr plate? If... |
I'm confused by what element(s) can be identified to have these properties.
The following is text from my 2019-2020 Kaplan MCAT General Chemistry book under the metalloids section
> *Silicon (Si) has a metallic luster but is brittle and a poor conductor*
So onto the MCAT Concept Check 2.2:
> Ident... |
What element has good conductivity but is also brittle? |
I'm confused by what element(s) can be identified to have these properties.
The following is text from my 2019-2020 Kaplan MCAT General Chemistry book under the metalloids section
> *Silicon (Si) has a metallic luster but is brittle and a poor conductor*
So onto the MCAT Concept Check 2.2:
> Identify a few ... |
You got oxidation numbers mixed up. As the comments pointed out, the +9 state is possible only in very few elements and mercury is not one of those.
To my understanding in general chemistry, this problem can easily solved using [Solubility Rules](https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemi... |
Has anyone seen a comparative list of typical run times of the techniques used in analytical chemistry? I am making a list of *rough* timescales of analytical techniques (for a slide). Assume that the sample preparation is aleady done.
For example:
Volumetric titration may take up to 10 minutes
Gravimetry can t... |
How many mutually immiscible liquids can be stored in a glass bottle at S.T.P.?
According to
> PATTLE, R. E. (1950). Systems of Mutually Immiscible Liquid Layers. Nature, 165(4188), 203–204.
a system of 6 immiscible phases can be formed (including Mercury), but the ammonia layer disappears after a month. They... |
How many mutually immiscible liquids can be stored in a glass bottle at S.T.P.?
According to
> PATTLE, R. E. (1950). Systems of Mutually Immiscible Liquid Layers. Nature, 165(4188), 203–204.
a system of 6 immiscible phases can be formed (including mercury), but the ammonia layer disappears after a month. They... |
In a neutral atom, can neutrons be ejected, and if so, by what (nuclear) process or reaction? For example, neutrons being ejected from lead-208 so that it is lead-197. |
Can neutrons be ejected from an atom? |
Answer key says that A is the most basic site but I don’t understand the concept behind that.
To assess the basic site, I’d normally look at the molecule as is and assess the current stability of the atom in question. The least stable would be my strongest base.
Looking at this question both the atoms properties ... |
Hydrazine $\ce{N2H4}$ and dinitrogen tetroxide $\ce{N2O4}$ form a hypergolic fuel and oxidizer pair widely used in spacecraft including [Akatsuki](https://en.wikipedia.org/wiki/Akatsuki_(spacecraft)).
Wikipedia [states](https://en.wikipedia.org/wiki/Hydrazine#Hydrazinium_salts):
>Hydrazine can be monoprotonated ... |
Piperine was chemically characterized by reaction with acids. This was done by dropping concentrated HNO3, HCl, and H2SO4 to a sample of piperine. Both HNO3 and HCl produced yellow solutions while Sulfuric acid produced a blood-red solution. What happens to piperine as it reacted with H2SO4 and why it turned blood-red?... |
What is the reaction between piperine and concentrated sulfuric acid? |
If I add a solute that decreases the bond strength of the pure solvent then wouldn't the solvent molecules evaporate more easily as it has lesser force holding it down now?But in my textbook, it's written that BP always increases when we add a non-volatile solute. |
why does adding a non volatile solute not decrease the boiling point? |
What is the right way to calculate the concentration of volatile compounds in the air in a closed container?
Suppose we have a $50\ mL$ bottle with $25\ mL$ of $100\ %$ ethanol (EtOH) in it.
In this case, will it be okay to use $PV=nRT$ ?
Doing so, it will be:
$$P_{EtOH} = 0.05872\ atm$$
$$V = 0.025\ L$$
... |
The azeotrope forming because of the hydrogen bond and the water and ethanol will evaporate together at the specific temperature. But before the specific temperature, even if the temperature doesn't reach the boiling point of the mixture, we know that there are still some ethanol evaporate. In this time(before the boil... |
Will there be some ethanol evaporating before the boiling point of ethanol? And will it bring some water with it because of the hydrogen bond? |
Expecting ideal gas behaviour $pV = nRT$ is not reasonable. Ideal gases are not in equilibrium with their liquid phase.
There should be rather used a [real gas equation][1].The easiest to use is the [van Der Waals equation][2], but even that has significant error near condensation state.
Additionally, the sample(!... |
In my syllabus we only study about rate laws under the topic "Rates of reactions" but as I was interested in it I started to search about that topic. And then I found the Arrhenius equation which says $\ln k=\ln A-E/RT $. But according to this equation k (rate constant) doesn't have units because we are taking the natu... |
[Azeotropes][1] exist for miscible liquids with mixing enthalpy sufficiently different to zero, what leads to existence of either minimum or maximum of total vapour pressure for particular molar fractions.
It also leads to partial pressure not being linear function of the molar fraction, being a deviation from the [Ra... |
In a neutral atom, can neutrons be ejected, and if so, by what (nuclear) process or reaction? I have read [Neutron emission][1] and [Can a proton be ejected from an atom][2], but I don't understand how and if that would work for removing neutrons from a heavy atom such as lead-208. Can neutrons be ejected from lead-208... |
How would you interpret the IR spectrum of your product if it's peaks match the literature spectrum, but the signals are weak? Could the argument that the sample was very dilute and lots of water was in it work as a viable explanation?
What about in a scenario where the experimental IR spectrum has all necessary pea... |
What are possible explanations for weak IR signals? |
In my syllabus we only study about rate laws under the topic "Rates of reactions", but as I was interested in it, I started to search about that topic. And then I found the Arrhenius equation
$$\ln k = \ln A - \frac{E}{RT}.$$
But according to this equation rate constant $k$ doesn't have units because we are takin... |
Piperine was chemically characterized by reaction with acids. This was done by dropping concentrated $\ce{HNO3},$ $\ce{HCl},$ and $\ce{H2SO4}$ to a sample of piperine. Both $\ce{HNO3}$ and $\ce{HCl}$ produced yellow solutions while sulfuric acid produced a blood-red solution.
What happens to piperine as it reacted w... |
What is the right way to calculate the concentration of volatile compounds in the air in a closed container?
Suppose we have a $\pu{50 mL}$ bottle with $\pu{25 mL}$ of $100\%$ ethanol $(\ce{EtOH})$ in it.
In this case, will it be okay to use $PV = nRT?$
Doing so, it will be:
$$
\begin{align}
p(\ce{EtOH}) ... |
Expecting ideal gas behaviour $pV = nRT$ is not reasonable. Ideal gases are not in equilibrium with their liquid phase.
There should be rather used a [real gas equation][1].The easiest to use is the [van Der Waals equation][2], but even that has significant error near condensation state.
Additionally, the samp... |
Even without any calculation, it must be obvious from the partial pressure approx. $\pu{0.06 atm}$ that it should be about approx. $\pu{60000 ppm (V/V)}$, not some $\pu{110 ppm}$.
Expecting ideal gas behaviour $pV = nRT$ is not reasonable. Ideal gases are not in equilibrium with their liquid phase.
There shoul... |
How is the ln k term in the linearised Arrhenius equation acceptable? |
Even without any calculation, it must be obvious from the partial pressure approx. $\pu{0.06 atm}$ that it should be about approx. $\pu{60000 ppm (V/V)}$, not some $\pu{110 ppm}$.
Usage of ppm/ppb etc units is discouraged, as they are ambiguous without the explicit context. As generally, 1 ppm (w/w) <> 1 ppm (V/V) <>... |
I was reacting **pure sodium and water**, and at one point I put some splattered sodium back into the water that had already been reacted with a pencil eraser size chunk of sodium. All of a sudden a bunch of "smoke" (visible fumes) was produced, and I breathed some of it in. **It burned my throat and nose**, so I left ... |
Sodium + water reaction, noxious fumes? |
Piperine was chemically characterized by reaction with acids. This was done by dropping concentrated $\ce{HNO3},$ $\ce{HCl},$ and $\ce{H2SO4}$ to a sample of piperine. Both $\ce{HNO3}$ and $\ce{HCl}$ produced yellow solutions while sulfuric acid produced a blood-red solution.
What happens to piperine as it reacted w... |
Question about HRMS:Phosphatidylcholines and phosphatidylethanolamines are common types of glycerophospholipids found in biological membranes. Because of the high amount of heteroatom content, electron impact mass spectrometry is a bad idea because the ions fragment too fast. For biological molecules, electrospray ioni... |
How do I explain the existence of these 2 peaks in this mass spectrometry? |
Or it actually blocks the oxidation? I read in some forum somewhere that to prevent Fe2+ from oxidizing, one should acidify the solution. Idk if that's the reason why we added H2SO4 in our Fe2+ solution. But then again, isnt Fe(II) unstable in the presence of acid and water? And will oxidize?
Imma tell yall my prof ... |
Can concentrated (18M) H2SO4 oxidize Fe2+ to Fe3+? |
Can concentrated (18M) H2SO4 oxidize Fe2+ to Fe3+? It actually blocks the oxidation? I read in some forum somewhere that to prevent Fe2+ from oxidizing, one should acidify the solution. Idk if that's the reason why we added H2SO4 in our Fe2+ solution. But then again, isnt Fe(II) unstable in the presence of acid and wat... |
I am developing a new type for the velocity of a reaction. This is the type I have developed so far:
u = A*n/m^2*(m1(u1)^2+m2(u2)^2)/Eact n*s.
where u is the reaction velocity
A = the common area of the substances
n/m^2 = the moles per square metre of each substance
u1 and u2 = average velocity of mo... |
I am developing a new type for the velocity of a reaction. This is the type I have developed so far:
$$u = A \times \frac{n}{m^2} \times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}} n \times s $$
where $u$ is the reaction velocity
$A =$ the common area of the substances
$n/m^2 =$ the moles per square metre... |
I am developing a new type for the velocity of a reaction. This is the type I have developed so far:
$$u = A \times \frac{n}{m^2} \times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}} $$ moles*sec
where $u$ is the reaction velocity
$A =$ the common area of the substances
$n/m^2 =$ the moles per square metre... |
I am developing a new type for the velocity of a reaction. This is the type I have developed so far:
$$u = A \times \frac{n}{m^2} \times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}} $$
where $u$ is the reaction velocity in $\pu{mol sec-1}$.
$A =$ the common area of the substances
$n/m^2 =$ the moles per ... |
Before the specific temperature, even if the temperature doesn't reach the boiling point of azeotrope or ethanol or water, we know that there are still some ethanol evaporate. In this time(before the boiling point of azeotrope(because the boiling point of azeotrope is the smallest)), will there be some water come out w... |
Will there be some ethanol evaporating before the boiling point of azeotrope? And will it bring some water with it because of the hydrogen bond? |
I am developing a new type for the velocity of a reaction. This is the type I have developed so far:
$$u = A \times \frac{n}{m^2} \times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}}\times 1/t $$
where $u$ is the reaction velocity in $\pu{mol sec-1}$.
$A =$ the common area of the substances
$n/m^2 =$ the moles... |
Why is the H−C−H bond angle in сhloromethane larger than 109.5°? |
Can concentrated (18 M) $\ce{H2SO4}$ oxidize $\ce{Fe^2+}$ to $\ce{Fe^3+}?$ Or does it actually block the oxidation? I read in some forum somewhere that in order to prevent $\ce{Fe^2+}$ from being oxidized, one should acidify the solution. I don't know if that's the reason why we added $\ce{H2SO4}$ in our $\ce{Fe^2+}$ s... |
Can concentrated sulfuric acid oxidize iron(II) to iron(III)? |
*Sorry for the possibly wrong terminology. I'm not a chemist and I'm not a native English speaker.
Please edit the question as needed. Thank you.*
Is it possible to buy or prepare a dispersion with the following properties?
- the particles should be >0.1μm in size, for example 0.11μm - 0.2μm
- there must be... |
A qualitative way to understand this trend is that with each increase in **n**, going row by row down a column, the electrons of filled inner shells create a screening effect upon the charge of the nucleus. The nuclear charge grows with each added proton, but as electrons are placed into new shells (with larger **n**) ... |
I am developing a new type for the velocity of a reaction. This is the type I have developed so far:
$$u = A \times \frac{n}{m^2} \times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}}\times 1/t $$
where $u$ is the rate of reaction in $\pu{mol sec-1}$.
$A =$ the common area of the substances
$n/m^2 =$ the moles ... |
I want to relate the macroscopic advancement of a reaction, the rate of the reaction, with the microscopic collisions of the molecules. This is the type I have developed so far:
$$u = A \times \frac{n}{m^2} \times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}}\times 1/t $$
where $u$ is the rate of reaction in $\pu{mo... |
I was wondering if I could please get some help with this:
" In a coffee cup calorimeter 100.oml of 1.0M NaOH and 100.0ml of 1.0M HCl are mixed. Both solutions are originally at 24.6C. After the reaction, the temperature is 31.3C. Assuming all solutions have a density of 1.0g/cm^3 and a specific heat capacity of 4.181... |
It is interesting to see you creating your own approach. The comments above provide good responses. I would recommend looking at Buttonwoods suggestion regarding collision theory and cross-sections. However, it appears none have answered your question directly, so I will provide my response to it here.
**Question:**... |
It is interesting to see you creating your own approach. The comments above provide good responses. I would recommend looking at Buttonwoods suggestion regarding collision theory and cross-sections. However, it appears none have answered your question directly, so I will provide my response to it here.
**Question:**... |
It is interesting to see you creating your own approach. The comments above provide good responses. I would recommend looking at Buttonwoods suggestion regarding collision theory and cross-sections. However, it appears none have answered your question directly, so I will provide my response to it here.
**Question:**... |
**Consider the two following cases**
***Case 1: Two Same Products***
Given the following chemical reaction,
$$A + B \rightarrow C + C$$
where C are radicals, therefore I am not writing $2C$ on the right hand side.
If we are to write the rate equation for the above expression, which one of the following... |
>***Case 2: Two Same Reactants***
$$2A + B \rightarrow C$$
Are the following correct?
$$\frac{d[A]}{dt} = -2k \cdot [A][B]$$
$$\frac{d[B]}{dt} = -k \cdot [A][B]$$
$$\frac{d[C]}{dt} = 2k \cdot [A][B]$$
Let's call $k \cdot [A][B]$ the rate. Your equations simplify to:
$$\frac{d[A]}{dt} = -2 \cdot \mathrm{rate}... |
We were assigned to prepare a standard Fe for spectrophotometry determination of Fe. What we did is basically obtain a mass of FeSO4•7H2O, add a small a mount of distilled water before adding 18M of H2SO4 then dilute.
My question is what exactly is the purpose of H2SO4? I asked my prof about it and she said it was ... |
I conducted an experiment to separate methanol and water. I am trying to determine the mole fraction of the distillate collected but having a little trouble with the calculation.
So i had a flow rate of 55ml/min. When i collected my sample i got a specific density of 0.815 and a volume of 334ml. I tried to work ou... |
A neighbour has been harassing us for eight years. Our property is lower than him. Last summer his newest craze was putting a hose up against the bordering fence and leaving it on, flooding us out below. It was easy to know it was due to the hose as last summer was the driest for a while in the UK.
All winter nothin... |
In computational chemistry of transition metals, there are many popular basis sets, from pople+LANL2DZ mixed basis sets, to Ahlrich and Karlsruhe basis sets like def-SVPD, def2-TZVPPD. Often the ECP versions of these basis sets were used to minimise computational expenses. However there are molecular properties such as... |
How to find a full electron basis set that approximate a given ECP basis set? |
Which pathway is better for robinson cycloaddition? 2-phenylacetaldehyde + 3-buten-2-one or 2-phenyl-2-propenal + acetone? |
I was offered the standard explanation that lone pairs are larger back in high school but in the first year of uni that was overturned by a pretty simple counterexample: the heavier homologues $\ce{H2S, PH3}$. While $\ce{SiH4}$ remains tetrahedral and has a similar orbital structure to $\ce{CH4}$, the bond angles in [$... |
Is there any home way of testing for tap water rather than rain water in the UK?
If not, is there any cheap way of getting someone else to test it?
A neighbour has been harassing us for eight years. Our property is lower than him. Last summer his newest craze was putting a hose up against the bordering fence and ... |
Is there any home way of testing for tap water rather than rain water in the UK?
If not, is there any cheap way of getting someone else to test it?
A neighbour has been harassing us for eight years. Our property is lower than him. Last summer his newest craze was putting a hose up against the bordering fence and ... |
*I apologize in advance for the large amount of text and thank all those who take the time to read it.*
----------
The "Click" reaction after Fokin and Sharpless is known to achieve high yields without long reaction times or harsh reaction conditions. The reaction is used mainly because of its high selectivit... |
*I apologize in advance for the large amount of text and thank all those who take the time to read it.*
----------
The "Click" reaction after Fokin and Sharpless is known to achieve high yields without long reaction times or harsh reaction conditions. The reaction is used mainly because of its high selectivit... |
I was wondering if I could please get some help with this:
" In a coffee-cup calorimeter 100.0 mL of 1.0 M $\ce{NaOH}$ and 100.0 mL of 1.0 M $\ce{HCl}$ are mixed. Both solutions are originally at 24.6 °C. After the reaction, the temperature is 31.3 °C. Assuming all solutions have a density of 1.0 g/cm<sup>3</sup> and ... |
I was wondering if I could please get some help with this:
> In a coffee-cup calorimeter $\pu{100.0 mL}$ of $\pu{1.0 M}~ \ce{NaOH}$ and $\pu{100.0 mL}$ of $\pu{1.0 M}\ \ce{HCl}$ are mixed. Both solutions are originally at $\pu{24.6 °C}$. After the reaction, the temperature is $\pu{31.3 °C}$. Assuming all solutions hav... |
I was wondering if I could please get some help with this:
> In a coffee-cup calorimeter $\pu{100.0 mL}$ of $\pu{1.0 M}~ \ce{NaOH}$ and $\pu{100.0 mL}$ of $\pu{1.0 M}\ \ce{HCl}$ are mixed. Both solutions are originally at $\pu{24.6 °C}$. After the reaction, the temperature is $\pu{31.3 °C}$. Assuming all solutions hav... |
I have read that vapour pressure of a mixture of two immiscible liquids is
$$P=P^0_A + P^0_B$$ where A and B are immiscible liquids.
If they are immiscible, they would form separate layers. Thus since the more dense liquid would be below the less dense liquid, it would have no interface with the gas phase. Given t... |
I was looking at the enthalpy of various liquids using WolframAlpha and noticed that at 30 °C, while water and ethanol have a positive enthalpy, acetone has a negative enthalpy.
If I'm understanding this correctly, this means that as acetone evaporates, the temperature of the acetone will *increase* (because the eva... |
I want to relate the macroscopic advancement of a reaction, the rate of the reaction, with the microscopic collisions of the molecules. This is the type I have developed so far:
$$u = A^2 \times \frac{n_1}{m^2} \times\frac{n_2}{m^2}\times \frac{(m_1u_1^2+m_2u_2^2)}{E_\mathrm{act}}\times 1/t $$
where $u$ is the ra... |
I was wondering if I could please get some help with this:
> In a coffee-cup calorimeter $\pu{100.0 mL}$ of $\pu{1.0 M}\ \ce{NaOH}$ and $\pu{100.0 mL}$ of $\pu{1.0 M}\ \ce{HCl}$ are mixed. Both solutions are originally at $\pu{24.6 ^\circ C}$. After the reaction, the temperature is $\pu{31.3 ^\circ C}$. Assuming all s... |
I was reacting **pure sodium and tap water**, and at one point I put some splattered sodium back into the water. I observed fumes that reacted with my respiratory system, producing a burning sensation.
I read that it is possible to produce sodium oxide fumes from sodium hydroxide at high temperatures (the sodium did... |
At equilibrium
$$ K=exp \left(\cfrac{TΔS^o-ΔH^o}{RT} \right) $$
$$ ⇒ \frac{lnK}{dT} = \frac{ΔH^o}{RT^2} $$
If enthalpy change is positive, change in lnK w.r.t. T is positive. Hence, lnK and therefore K increase (position of equilibrium shifts to the right) as T increases. And, lnK and therefore K decrease (posit... |
Anti-aromatic compounds are formed with a cyclic system of planar, overlapping p orbitals containing a non-Huckel number of electrons (i.e. not 4n+2 electrons -n being a natural number-). Non-aromatic compounds do not contain a continuously overlapping cyclic system of p orbitals. If a compound is antiaromatic, it is g... |
What is the Criteria for a Compound Being Non-aromatic vs. Anti-aromatic? |
Anti-aromatic compounds are formed with a cyclic system of planar, overlapping p orbitals containing a non-Huckel number of electrons (i.e. not 4n+2 electrons -n being a natural number-). Non-aromatic compounds do not contain a continuously overlapping cyclic system of p orbitals. If a compound is antiaromatic, it is g... |
The reaction of the ketal **1** with aqueous H<sub>2</sub>SO<sub>4</sub> is most likely to follow the pathway **1** --> **2** --> **3** to form α,β-unsaturated ketone **3**. This is a typical ketal hydrolysis in acid medium. For the proposed reaction pathway **1** --> **4** --> **5** --> **6**, species **6**... |
At equilibrium
$$
\begin{align}
K &= \exp\left(\cfrac{TΔS^\circ - ΔH^\circ}{RT}\right)\\
⇒ \frac{\ln K}{\mathrm dT} &= \frac{ΔH^\circ}{RT^2}
\end{align}
$$
If enthalpy change is positive, change in $\ln K$ w.r.t. $T$ is positive. Hence, $\ln K$ and therefore $K$ increase (position of equilibrium shifts to th... |
Usage of ppm/ppb etc units is discouraged, as they are ambiguous without the explicit context. As generally, 1 ppm (w/w) <> 1 ppm (V/V) <> 1 ppm (n/n) <> 1 ppm (w/V).
It is recommended to use explicit units, like e.g mg/L.
Expecting ideal gas behaviour $pV = nRT$ is not reasonable. Ideal gases are not in equili... |
My textbook states that because $sp^2-sp^3$ bonds are stronger than $sp^3-sp^3$ bonds, alkenes are more stable than alkanes. The rule given is that bonds with more $s$ character are stronger.
However, it then states that an alkene with more alkyl substituents at the C=C double bond is stronger than an alkene with ju... |
Why do alkyl substituents stabilize alkenes? |
In typical software like Gaussian or GAMESS, the molecular orbitals (or even the basis functions) can be displayed as surfaces.
I understand that the surface is probably constructed from a series of points that give a fixed value when substituted into the wavefunction. However, how are these points calculated? Sinc... |
How are orbitals displayed in computational Chemistry software? |
Standard state conditions for standard Gibbs energy change stipulate (among other conditions) that partial pressure of each gas = 1 bar.
e.g. 2A + 3B = 4C + 5D (all gases)
Then for standard Gibbs energy change calculations partial pressure of A or B or C or D is same = 1 bar.
What I want to know is that if we are c... |
A friend from customs said "if drugs have been in a glass jar for more than a day, the aromatic compounds travel through the lid and the dog can detect it, especially after 2-3 days. They can travel through almost any material given enough time"
Is that correct? Why so? |
Subsets and Splits
No community queries yet
The top public SQL queries from the community will appear here once available.