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or a base. for glycine, the acid strength of the carboxyl group is about the same as that of acetic acid, ch3co2h, and the base strength of the amino group is slightly greater than that of ammonia, nh3. ( a ) write the lewis structures of the ions that form when glycine is dissolved in 1 m hcl and in 1 m koh. ( b ) wri... | openstax_chemistry2e-web | [
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15. 3 coupled equilibria 85. a saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. explain. why is such a system called a heterogeneous equilibrium? 86. calculate the equilibrium concentration of ni2 + in a 1. 0 - m solution [ ni ( nh... | openstax_chemistry2e-web | [
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– 2. 96. what is the molar solubility of tl ( oh ) 3 in a 0. 10 - m solution of nh3? 97. what is the molar solubility of pb ( oh ) 2 in a 0. 138 - m solution of ch3nh2? 98. a solution of 0. 075 m cobr2 is saturated with h2s ( [ h2s ] = 0. 10 m ). what is the minimum ph at which cos begins to precipitate? 99. a 0. 125 -... | openstax_chemistry2e-web | [
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. 00 10 – 3 - m solution of mg ( no3 ) 2 is mixed with 200. 0 ml of a 2. 00 10 – 3 - m solution of naf at 18 °c. show the calculations to support your prediction. ( d ) at 27 °c the concentration of mg2 + in a saturated solution of mgf2 is 1. 17 10 – 3 m. is the dissolving of mgf2 in water an endothermic or an exotherm... | openstax_chemistry2e-web | [
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cahpo4 106. identify all chemical species present in an aqueous solution of ca3 ( po4 ) 2 and list these species in decreasing order of their concentrations. ( hint : remember that the ion is a weak base. ) 15 • exercises 781 782 15 • exercises access for free at openstax. org introduction chapter 16 thermodynamics 16.... | openstax_chemistry2e-web | [
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16. 1 spontaneity learning objectives by the end of this section, you will be able to : • distinguish between spontaneous and nonspontaneous processes • describe the dispersal of matter and energy that accompanies certain spontaneous processes figure 16. 1 geysers are a dramatic display of thermodynamic principles in n... | openstax_chemistry2e-web | [
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as they are converted to more stable nuclei. all the decay processes occur spontaneously, but the rates at which different isotopes decay vary widely. technetium - 99m is a popular radioisotope for medical imaging studies that undergoes relatively rapid decay and exhibits a half - life of about six hours. uranium - 238... | openstax_chemistry2e-web | [
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##asurably slow at low to moderate temperatures. this process is known as graphitization, and its rate can be increased to easily measurable values at temperatures in the 1000 – 2000 k range. ( credit " diamond " photo : modification of work by " fancy diamonds " / flickr ; credit " graphite " photo : modification of w... | openstax_chemistry2e-web | [
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to a | openstax_chemistry2e-web | [
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16. 1 • spontaneity 785 second flask containing a vacuum. once the valve is opened, the gas spontaneously becomes evenly distributed between the flasks. now consider two objects at different temperatures : object x at temperature tx and object y at temperature ty, with tx > ty ( figure 16. 5 ). when these objects come ... | openstax_chemistry2e-web | [
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since the molecules will occupy a much greater volume after the solid - to - gas transition. ( b ) condensation is the conversion of a gas ( relatively low density ) to a liquid ( much greater density ). this process yields a much lesser dispersal of matter, since the molecules will occupy a much lesser volume after 78... | openstax_chemistry2e-web | [
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16. 2 entropy learning objectives by the end of this section, you will be able to : • define entropy • explain the relationship between entropy and the number of microstates • predict the sign of the entropy change for chemical and physical processes in 1824, at the age of 28, nicolas leonard sadi carnot ( figure 16. 7... | openstax_chemistry2e-web | [
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16. 2 • entropy 787 the entropy change for a real, irreversible process is then equal to that for the theoretical reversible process that involves the same initial and final states. entropy and microstates following the work of carnot and clausius, ludwig boltzmann developed a molecular - scale statistical model that r... | openstax_chemistry2e-web | [
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is therefore the one of greatest entropy. figure 16. 8 the sixteen microstates associated with placing four particles in two boxes are shown. the microstates are collected into five distributions — ( a ), ( b ), ( c ), ( d ), and ( e ) — based on the numbers of particles in each box. for this system, the most probable ... | openstax_chemistry2e-web | [
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this particle - in - a - box model. for this system, the most probable distribution is confirmed to be the one in which the matter is most uniformly dispersed or distributed between the two flasks. initially, the gas molecules are confined to just one of the two flasks. opening the valve between the flasks increases th... | openstax_chemistry2e-web | [
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’ temperatures. and, again, this spontaneous process is also characterized by an increase in system entropy. figure 16. 9 this shows a microstate model describing the flow of heat from a hot object to a cold object. ( a ) before the heat flow occurs, the object comprised of particles a and b contains both units of ener... | openstax_chemistry2e-web | [
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16. 2 • entropy 789 example 16. 2 determination of δs calculate the change in entropy for the process depicted below. solution the initial number of microstates is one, the final six : the sign of this result is consistent with expectation ; since there are more microstates possible for the final state than for the ini... | openstax_chemistry2e-web | [
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substance increases ( δs > 0 ) as it transforms from a relatively ordered solid, to a less - ordered liquid, and then to a still less - ordered gas. the entropy decreases ( δs < 0 ) as the substance transforms from a gas to a liquid and then to a solid. now consider the gaseous phase, in which a given number of atoms o... | openstax_chemistry2e-web | [
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16. 2 • entropy 791 particle location and freedom of motion on physical state and temperature. the entropy of a substance is influenced by the structure of the particles ( atoms or molecules ) that comprise the substance. with regard to atomic substances, heavier atoms possess greater entropy at a given temperature tha... | openstax_chemistry2e-web | [
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net decrease in the amount of gaseous species ( d ) positive, phase transition from solid to liquid, net increase in dispersal of matter check your learning predict the sign of the entropy change for the following processes. give a reason for your prediction. ( a ) ( b ) the freezing of liquid water ( c ) ( d ) answer ... | openstax_chemistry2e-web | [
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16. 3 the second and third laws of thermodynamics learning objectives by the end of this section, you will be able to : • state and explain the second and third laws of thermodynamics • calculate entropy changes for phase transitions and chemical reactions under standard conditions the second law of thermodynamics in t... | openstax_chemistry2e-web | [
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: the arithmetic signs of qrev denote the gain of heat by the system and the loss of heat by the surroundings. the magnitude of the entropy change for the surroundings will again be greater than that for the system, but in this case, the signs of the heat changes ( that is, the direction of the heat flow ) will yield a... | openstax_chemistry2e-web | [
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16. 3 • the second and third laws of thermodynamics 793 the second law of thermodynamics δsuniv > 0 spontaneous δsuniv < 0 nonspontaneous ( spontaneous in opposite direction ) δsuniv = 0 at equilibrium table 16. 1 for many realistic applications, the surroundings are vast in comparison to the system. in such cases, the... | openstax_chemistry2e-web | [
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. check your learning using this information, determine if liquid water will spontaneously freeze at the same temperatures. what can you say about the values of suniv? 794 16 • thermodynamics access for free at openstax. org answer : entropy is a state function, so δsfreezing = −δsmelting = −22. 1 j / k and qsurr = + 6... | openstax_chemistry2e-web | [
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ν represents stoichiometric coefficients in the balanced equation representing the process. for example, δs° for the following reaction at room temperature is computed as : a partial listing of standard entropies is provided in table 16. 2, and additional values are provided in appendix g. the example exercises that fo... | openstax_chemistry2e-web | [
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205. 03 table 16. 2 standard entropies for selected substances measured at 1 atm and 298. 15 k. ( values are approximately equal to those measured at 1 bar, the currently accepted standard state pressure. ) example 16. 5 determination of δs° calculate the standard entropy change for the following process : solution cal... | openstax_chemistry2e-web | [
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16. 4 free energy learning objectives by the end of this section, you will be able to : • define gibbs free energy, and describe its relation to spontaneity • calculate free energy change for a process using free energies of formation for its reactants and products • calculate free energy change for a process using ent... | openstax_chemistry2e-web | [
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16. 4 • free energy 797 comparing this equation to the previous one for free energy change shows the following relation : the free energy change is therefore a reliable indicator of the spontaneity of a process, being directly related to the previously identified spontaneity indicator, δsuniv. table 16. 3 summarizes th... | openstax_chemistry2e-web | [
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so the work done by these processes is always less than the theoretical maximum. similar reasoning may be applied to a nonspontaneous process, for which the free energy change represents the minimum amount of work that must be done on the system to carry out the process. calculating free energy change free energy is a ... | openstax_chemistry2e-web | [
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188. 8 using the appendix data to calculate the standard enthalpy and entropy changes yields : substitution into the standard free energy equation yields : at 298 k ( 25 °c ) so boiling is nonspontaneous ( not spontaneous ). check your learning use standard enthalpy and entropy data from appendix g to calculate the sta... | openstax_chemistry2e-web | [
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205. 2 ( a ) using free energies of formation : ( b ) using enthalpies and entropies of formation : 800 16 • thermodynamics access for free at openstax. org both ways to calculate the standard free energy change at 25 °c give the same numerical value ( to three significant figures ), and both predict that the process i... | openstax_chemistry2e-web | [
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reaction exhibits a negative free energy change and is spontaneous : this process is typically carried out at elevated temperatures, so this result obtained using standard free energy values is just an estimate. the gist of the calculation, however, holds true. | openstax_chemistry2e-web | [
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16. 4 • free energy 801 example 16. 9 calculating free energy change for a coupled reaction is a reaction coupling the decomposition of zns to the formation of h2s expected to be spontaneous under standard conditions? solution following the approach outlined above and using free energy values from appendix g : the coup... | openstax_chemistry2e-web | [
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δs are negative. this condition describes an exothermic process that involves a decrease in system entropy. in this case, δg will be negative if the magnitude of the tδs term is less than δh. if the tδs term ’ s magnitude is greater than δh, the free energy change will be positive. such a process is spontaneous at low ... | openstax_chemistry2e-web | [
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at low temperatures. when considering the conclusions drawn regarding the temperature dependence of spontaneity, it is important to keep in mind what the terms “ high ” and “ low ” mean. since these terms are adjectives, the temperatures in question are deemed high or low relative to some reference temperature. a proce... | openstax_chemistry2e-web | [
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16. 4 • free energy 803 so, saying a process is spontaneous at “ high ” or “ low ” temperatures means the temperature is above or below, respectively, that temperature at which δg for the process is zero. as noted earlier, the condition of δg = 0 describes a system at equilibrium. figure 16. 13 these plots show the var... | openstax_chemistry2e-web | [
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process in the reverse direction. when δg is zero, the forward and reverse driving forces are equal, and the process occurs in both directions at the same rate ( the system is at equilibrium ). in the chapter on equilibrium the reaction quotient, q, was introduced as a convenient measure of the status of an equilibrium... | openstax_chemistry2e-web | [
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16. 4 • free energy 805 since the computed value for δg is positive, the reaction is nonspontaneous under these conditions. check your learning calculate the free energy change for this same reaction at 875 °c in a 5. 00 l mixture containing 0. 100 mol of each gas. is the reaction spontaneous under these conditions? an... | openstax_chemistry2e-web | [
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j. check your learning use the thermodynamic data provided in appendix g to calculate the equilibrium constant for the dissociation of dinitrogen tetroxide at 25 °c. answer : k = 6. 9 to further illustrate the relation between these two essential thermodynamic concepts, consider the observation that reactions spontaneo... | openstax_chemistry2e-web | [
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16. 4 • free energy 807 figure 16. 14 these plots show the free energy versus reaction progress for systems whose standard free energy changes are ( a ) negative, ( b ) positive, and ( c ) zero. nonequilibrium systems will proceed spontaneously in whatever direction is necessary to minimize free energy and establish eq... | openstax_chemistry2e-web | [
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at absolute zero ( 0 k ) is zero key equations s = k ln w δsuniv = δssys + δssurr δg = δh −tδs summary 16. 1 spontaneity chemical and physical processes have a natural tendency to occur in one direction under certain conditions. a spontaneous process occurs without the need for a continual input of energy from some ext... | openstax_chemistry2e-web | [
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16. 2 entropy entropy ( s ) is a state function that can be related to the number of microstates for a system ( the number of ways the system can be arranged ) and to the ratio of reversible heat to kelvin temperature. it may be interpreted as a measure of the dispersal or distribution of matter and / or energy in a sy... | openstax_chemistry2e-web | [
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of free energy changes are possible. exercises | openstax_chemistry2e-web | [
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16. 1 spontaneity 1. what is a spontaneous reaction? 2. what is a nonspontaneous reaction? 3. indicate whether the following processes are spontaneous or nonspontaneous. ( a ) liquid water freezing at a temperature below its freezing point ( b ) liquid water freezing at a temperature above its freezing point ( c ) the ... | openstax_chemistry2e-web | [
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16. 2 entropy 6. in figure 16. 8 all possible distributions and microstates are shown for four different particles shared between two boxes. determine the entropy change, δs, if the particles are initially evenly distributed between the two boxes, but upon redistribution all end up in box ( b ). 7. in figure 16. 8 all ... | openstax_chemistry2e-web | [
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l ), h2o ( g ), h2o ( s ) ( c ) he ( g ), cl2 ( g ), p4 ( g ) 13. at room temperature, the entropy of the halogens increases from i2 to br2 to cl2. explain. 14. consider two processes : sublimation of i2 ( s ) and melting of i2 ( s ) ( note : the latter process can occur at the same temperature but somewhat higher pres... | openstax_chemistry2e-web | [
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16. 3 the second and third laws of thermodynamics 20. what is the difference between δs and δs° for a chemical change? 21. calculate for the following changes. ( a ) ( b ) ( c ) ( d ) ( e ) ( f ) ( g ) 22. determine the entropy change for the combustion of liquid ethanol, c2h5oh, under the standard conditions to give g... | openstax_chemistry2e-web | [
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( f ) | openstax_chemistry2e-web | [
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16. 4 free energy 30. what is the difference between δg and δg° for a chemical change? 31. a reaction has = 100 kj / mol and is the reaction spontaneous at room temperature? if not, under what temperature conditions will it become spontaneous? 32. explain what happens as a reaction starts with δg < 0 ( negative ) and r... | openstax_chemistry2e-web | [
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conditions as suitable candidates for fuels. ( a ) ammonia : ( b ) diborane : ( c ) hydrazine : ( d ) hydrogen peroxide : 39. calculate δg° for each of the following reactions from the equilibrium constant at the temperature given. ( a ) ( b ) ( c ) ( d ) ( e ) ( f ) 40. calculate δg° for each of the following reaction... | openstax_chemistry2e-web | [
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standard free energy change for the aqueous reaction of hydrogen ion with hydroxide ion to produce water. ( hint : the reaction is the reverse of the self - ionization reaction. ) 49. hydrogen sulfide is a pollutant found in natural gas. following its removal, it is converted to sulfur by the reaction what is the equil... | openstax_chemistry2e-web | [
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acetic acid, ch3co2h, can form a dimer, ( ch3co2h ) 2, in the gas phase. the dimer is held together by two hydrogen bonds with a total strength of 66. 5 kj per mole of dimer. at 25 °c, the equilibrium constant for the dimerization is 1. 3 103 ( pressure in atm ). what is δs° for the reaction? 814 16 • exercises access ... | openstax_chemistry2e-web | [
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respect to the enthalpy and entropy changes. explain why diamond spontaneously changing into graphite is not observed. 60. the evaporation of one mole of water at 298 k has a standard free energy change of 8. 58 kj. ( a ) is the evaporation of water under standard thermodynamic conditions spontaneous? ( b ) determine t... | openstax_chemistry2e-web | [
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the temperature is 37 °c. 63. without doing a numerical calculation, determine which of the following will reduce the free energy change for the reaction, that is, make it less positive or more negative, when the temperature is increased. explain. ( a ) ( b ) ( c ) ( d ) 64. when ammonium chloride is added to water and... | openstax_chemistry2e-web | [
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17. 7 electrolysis another chapter in this text introduced the chemistry of reduction - oxidation ( redox ) reactions. this important reaction class is defined by changes in oxidation states for one or more reactant elements, and it includes a subset of reactions involving the transfer of electrons between reactant spe... | openstax_chemistry2e-web | [
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17. 1 review of redox chemistry learning objectives by the end of this section, you will be able to : • describe defining traits of redox chemistry • identify the oxidant and reductant of a redox reaction • balance chemical equations for redox reactions using the half - reaction method since reactions involving electro... | openstax_chemistry2e-web | [
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, + 2 and −1, respectively. covalent compounds require a more challenging use of the formalism. water is a covalent compound whose molecules consist of two h atoms bonded separately to a central o atom via polar covalent o−h bonds. the shared electrons comprising an o−h bond are more strongly attracted to the more elec... | openstax_chemistry2e-web | [
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##ox reactions that take place in aqueous solutions are commonly encountered in electrochemistry, and many involve water or its characteristic ions, h + ( aq ) and oh− ( aq ), as reactants or products. in these cases, equations representing the redox reaction can be very challenging to balance by inspection, and the us... | openstax_chemistry2e-web | [
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adding electrons. 6. if necessary, multiply one or both half - reactions so that the number of electrons consumed in one is equal to the number produced in the other. 7. add the two half - reactions and simplify. 8. if the reaction takes place in a basic medium, add oh−ions the equation obtained in step 7 to neutralize... | openstax_chemistry2e-web | [
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17. 1 • review of redox chemistry 819 this step not necessary since the solution is stipulated to be acidic. the balanced equation for the reaction in an acidic solution is then check your learning the reaction above results when using relatively diluted nitric acid. if concentrated nitric acid is used, nitrogen dioxid... | openstax_chemistry2e-web | [
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ion, bro3−. write the balanced equation for this 820 17 • electrochemistry access for free at openstax. org reaction occurring in a basic medium. answer : | openstax_chemistry2e-web | [
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17. 2 galvanic cells learning objectives by the end of this section, you will be able to : • describe the function of a galvanic cell and its components • use cell notation to symbolize the composition and construction of galvanic cells as demonstration of spontaneous chemical change, figure 17. 2 shows the result of i... | openstax_chemistry2e-web | [
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i ) is depicted in figure 17. 3. the cell is comprised of two half - cells, each containing the redox conjugate pair ( “ couple ” ) of a single reactant. the half - cell shown at the left contains the cu ( 0 ) / cu ( ii ) couple in the form of a solid copper foil and an aqueous solution of copper nitrate. the right hal... | openstax_chemistry2e-web | [
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17. 2 • galvanic cells 821 figure 17. 3 a galvanic cell based on the spontaneous reaction between copper and silver ( i ) ions. cell notation abbreviated symbolism is commonly used to represent a galvanic cell by providing essential information on its composition and structure. these symbolic representations are called... | openstax_chemistry2e-web | [
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then written as notice the cathode half - cell is different from the others considered thus far in that its electrode is comprised of a substance ( pt ) that is neither a reactant nor a product of the cell reaction. this is required when neither member of the half - cell ’ s redox couple can reasonably function as an e... | openstax_chemistry2e-web | [
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learning omitting solute concentrations and spectator ion identities, write the schematic for a galvanic cell whose net cell reaction is shown below. answer : | openstax_chemistry2e-web | [
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17. 3 electrode and cell potentials learning objectives by the end of this section, you will be able to : • describe and relate the definitions of electrode and cell potentials • interpret electrode potentials in terms of relative oxidant and reductant strengths • calculate cell potentials and predict redox spontaneity... | openstax_chemistry2e-web | [
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, defined as where ecathode and eanode are the potentials of two different half - cells functioning as specified in the subscripts. as for other thermodynamic quantities, the standard cell potential, e°cell, is a cell potential measured when both half - cells are under standard - state conditions ( 1 m concentrations, ... | openstax_chemistry2e-web | [
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the potential difference between the two half - cells. since the cu half - cell is designated as the cathode in the definition of cell potential, it is connected to the red ( positive ) input of the voltmeter, while the designated she anode is connected to the black ( negative ) input. these connections insure that the... | openstax_chemistry2e-web | [
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17. 3 • electrode and cell potentials 825 figure 17. 6 a cell permitting experimental measurement of the standard electrode potential for the half - reaction table 17. 1 provides a listing of standard electrode potentials for a selection of half - reactions in numerical order, and a more extensive alphabetical listing ... | openstax_chemistry2e-web | [
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17. 3 • electrode and cell potentials 827 half - reaction e° ( v ) −2. 868 −2. 912 −2. 931 −3. 04 table 17. 1 example 17. 4 calculating standard cell potentials what is the standard potential of the galvanic cell shown in figure 17. 3? solution the cell in figure 17. 3 is galvanic, the spontaneous cell reaction involvi... | openstax_chemistry2e-web | [
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half - reaction is a weaker oxidant than aqueous hydrogen ions. 828 17 • electrochemistry access for free at openstax. org applying this logic to the numerically ordered listing of standard electrode potentials in table 17. 1 shows this listing to be likewise in order of the oxidizing strength of the half - reaction ’ ... | openstax_chemistry2e-web | [
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opposite direction. as an indicator of spontaneity for redox reactions, the potential of a cell reaction shows a consequential relationship in its arithmetic sign. the spontaneous oxidation of copper by lead ( ii ) ions is not observed, and so the reverse reaction, the oxidation of lead by copper ( ii ) ions, is predic... | openstax_chemistry2e-web | [
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##de ion by molecular bromine. answer : | openstax_chemistry2e-web | [
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17. 4 potential, free energy, and equilibrium learning objectives by the end of this section, you will be able to : • explain the relations between potential, free energy change, and equilibrium constants • perform calculations involving the relations between cell potentials, free energy changes, and equilibrium • use ... | openstax_chemistry2e-web | [
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chapter on thermodynamics ) and the equation above relating δg° and e°cell yields the following : this equation indicates redox reactions with large ( positive ) standard cell potentials will proceed far towards completion, reaching equilibrium when the majority of reactant has been converted to product. a summary of t... | openstax_chemistry2e-web | [
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17. 4 • potential, free energy, and equilibrium 831 the standard free energy is then the reaction is spontaneous, as indicated by a negative free energy change and a positive cell potential. the k value is very large, indicating the reaction proceeds to near completion to yield an equilibrium mixture containing mostly ... | openstax_chemistry2e-web | [
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electrochemistry access for free at openstax. org solution collecting information from appendix l and the problem, notice the negative value of the standard cell potential indicates the process is not spontaneous under standard conditions. substitution of the nernst equation terms for the nonstandard conditions yields ... | openstax_chemistry2e-web | [
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17. 4 • potential, free energy, and equilibrium 833 the positive value for cell potential indicates the overall cell reaction ( see above ) is spontaneous. this spontaneous reaction is one in which the zinc ion concentration in the cathode falls ( it is reduced to elemental zinc ) while that in the anode rises ( it is ... | openstax_chemistry2e-web | [
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17. 5 batteries and fuel cells learning objectives by the end of this section, you will be able to : • describe the electrochemistry associated with several common batteries • distinguish the operation of a fuel cell from that of a battery there are many technological products associated with the past two centuries of ... | openstax_chemistry2e-web | [
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primary battery is the dry cell, which uses a zinc can as both container and anode ( “ – ” terminal ) and a graphite rod as the cathode ( “ + ” terminal ). the zn can is filled with an electrolyte paste containing manganese ( iv ) oxide, zinc ( ii ) chloride, ammonium chloride, and water. a graphite rod is immersed in ... | openstax_chemistry2e-web | [
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17. 5 • batteries and fuel cells 835 and they were designed around the same redox couples. as their name suggests, these types of batteries use alkaline electrolytes, often potassium hydroxide. the reactions are an alkaline battery can deliver about three to five times the energy of a zinc - carbon dry cell of similar ... | openstax_chemistry2e-web | [
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##d batteries use a “ jelly - roll ” design that significantly increases the amount of current the battery can deliver as compared to a similar - sized alkaline battery. link to learning visit this site ( http : / / openstax. org / l / 16nicdrecharge ) for more information about nickel cadmium rechargeable batteries. l... | openstax_chemistry2e-web | [
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17. 5 • batteries and fuel cells 837 figure 17. 12 in a lithium ion battery, charge flows as the lithium ions are transferred between the anode and cathode. link to learning visit this site ( http : / / openstax. org / l / 16lithiumion ) for more information about lithium ion batteries. the lead acid battery ( figure 1... | openstax_chemistry2e-web | [
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reactions : figure 17. 14 in this hydrogen fuel cell, oxygen from the air reacts with hydrogen, producing water and electricity. these types of fuel cells generally produce voltages of approximately 1. 2 v. compared to an internal combustion engine, the energy efficiency of a fuel cell using the same redox reaction is ... | openstax_chemistry2e-web | [
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17. 6 corrosion learning objectives by the end of this section, you will be able to : • define corrosion • list some of the methods used to prevent or slow corrosion corrosion is usually defined as the degradation of metals by a naturally occurring electrochemical process. the formation of rust on iron, tarnish on silv... | openstax_chemistry2e-web | [
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for free at openstax. org perhaps the most familiar example of corrosion is the formation of rust on iron. iron will rust when it is exposed to oxygen and water. rust formation involves the creation of a galvanic cell at an iron surface, as illustrated in figure 17. 15. the relevant redox reactions are described by the... | openstax_chemistry2e-web | [
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17. 6 • corrosion 841 figure 17. 16 corrosion can occur when a painted iron or steel surface is exposed to the environment by a scratch through the paint. a galvanic cell results that may be approximated by the simplified cell schematic fe ( s ) | fe2 + ( aq ) | | o2 ( aq ), h2o ( l ) | fe ( s ). one way to keep iron f... | openstax_chemistry2e-web | [
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( lower reduction potential ) are called sacrificial anodes because as they get used up as they corrode ( oxidize ) at the anode. the metal being protected serves as the cathode for the reduction of oxygen in air, and so it simply serves to conduct ( not react with ) the electrons being transferred. when the anodes are... | openstax_chemistry2e-web | [
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17. 7 electrolysis learning objectives by the end of this section, you will be able to : • describe the process of electrolysis • compare the operation of electrolytic cells with that of galvanic cells • perform stoichiometric calculations for electrolytic processes electrochemical cells in which spontaneous redox reac... | openstax_chemistry2e-web | [
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reaction, a positive potential of magnitude greater than the negative cell potential must be applied to the cell. | openstax_chemistry2e-web | [
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17. 7 • electrolysis 843 figure 17. 18 cells of this sort ( a cell for the electrolysis of molten sodium chloride ) are used in the downs process for production of sodium and chlorine, and they typically use iron cathodes and carbon anodes. the electrolysis of water water may be electrolytically decomposed in a cell si... | openstax_chemistry2e-web | [
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##rmodynamics thus predicts that water would be more readily oxidized, though in practice it is observed that both water and chloride ion are oxidized under typical conditions, producing a mixture of oxygen and chlorine gas. turning attention to the cathode, the possibilities for reduction are : comparison of these sta... | openstax_chemistry2e-web | [
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17. 7 • electrolysis 845 thermodynamically favored. however, in a neutral aqueous sodium chloride solution, the concentration of hydrogen ion is far below the standard state value of 1 m ( approximately 10 - 7 m ), and so the observed cathode reaction is actually reduction of water. the net cell reaction in this case i... | openstax_chemistry2e-web | [
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right and is the spoon, which is made from inexpensive metal. both electrodes are immersed in a solution of silver nitrate. applying a sufficient potential results in the oxidation of the silver anode and reduction of silver ion at the ( spoon ) cathode : the net result is the transfer of silver metal from the anode to... | openstax_chemistry2e-web | [
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. 9 g / mol, so check your learning aluminum metal can be made from aluminum ( iii ) ions by electrolysis. what is the half - reaction at the cathode? what mass of aluminum metal would be recovered if a current of 25. 0 a passed through the solution for 15. 0 minutes? answer : 0. 0777 mol al = 2. 10 g al. example 17. 1... | openstax_chemistry2e-web | [
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11. 8 kg zn requires 382 hours. 848 17 • electrochemistry access for free at openstax. org key terms active electrode electrode that participates as a reactant or product in the oxidation - reduction reaction of an electrochemical cell ; the mass of an active electrode changes during the oxidation - reduction reaction ... | openstax_chemistry2e-web | [
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/ mol e− fuel cell devices similar to galvanic cells that require a continuous feed of redox reactants ; also called a flow battery galvanic ( voltaic ) cell electrochemical cell in which a spontaneous redox reaction takes place ; also called a voltaic cell galvanization method of protecting iron or similar metals from... | openstax_chemistry2e-web | [
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hydrogen ion production, assigned a potential of exactly 0 v under standard state conditions, used as the universal reference for measuring electrode potential 17 • key terms 849 key equations δg = −nfecell q = i t = n f summary 17. 1 review of redox chemistry redox reactions are defined by changes in reactant oxidatio... | openstax_chemistry2e-web | [
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17. 3 electrode and cell potentials the property of potential, e, is the energy associated with the separation / transfer of charge. in electrochemistry, the potentials of cells and half - cells are thermodynamic quantities that reflect the driving force or the spontaneity of their redox processes. the cell potential o... | openstax_chemistry2e-web | [
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