Question

In: Chemistry

1-1Based on the Gibbs free energy of formation of substances listed in the table below, calculate...

1-1Based on the Gibbs free energy of formation of substances listed in the table below, calculate EMF for the following cells:

(i) Zn | Zn2+ (1.0 M) || H+ (1.0 M) | O2 (1 atm) | Pt

(ii) Zn | Zn2+ (1.0 M) || Cu2+ (1.0 M) | Cu

(iii) Pt | H2(g) (1 atm) | H+ (1.0 M) || H+ (1.0 M) | O2 (1 atm) | Pt

_______________________________________________

Substances                               DGfo/ kJ mol-1 (298 K)

_______________________________________________

Zn2+(aq)                                  -147.0

ZnO(s)                                     -318.3

Mn2+(aq)                                 -228.3

MnO4-(aq)                               -447.3

MnO2(s)                                  -465.2

Mn2O3(s)                                 -881.15

OH-(aq)                                   -157.2

H2O(l)                                     -237.1

Cu2+(aq)                                  +65.52

Cu+(aq)                                    +50.0

Fe3+(aq)                                   -4.6

Fe2+(aq)                                   -78.87

Cr3+(aq)                                   -197.05

CrO42-(aq)                               -727.8

Cr2O72-(aq)                             -1301.2

Ce3+(aq)                                  -672.0

Ce4+(aq)                                  -533.06

Ag+(aq)                                   +77.12

AgCl(s)                                   -109.8

Cl-(aq)                                     -131.3

_______________________________________________

Solutions

Expert Solution

queen_honey_blossom answered 9 months ago
Next > < Previous

Related Solutions

Using standard Gibbs energy of formation values given in the table, calculate the equilibrium constant K...
Using standard Gibbs energy of formation values given in the table, calculate the equilibrium constant K of the reaction Cl2(g)+2NO(g)⇌2NOCl(g) The standard Gibbs energy change of the reaction represents the drive the reaction has under standard conditions to move toward equilibrium from point A to point X in the diagram. Substance ΔfG∘ (kJ mol−1) Cl2(g) 0 NO(g) 86.71 NOCl(g) 66.30
1. Calculate the standard reaction entropy, enthalpy and Gibbs free energy for the following reactions a)...
1. Calculate the standard reaction entropy, enthalpy and Gibbs free energy for the following reactions a) N2(g) + NO2(g) ---> NO(g) + N2O(g) and b) 2F2(g) +2H2O(l) ---> 4HF(aq) + O2(g)
Consider the following reaction and calculate the standard Gibbs Free Energy for it. 2 NO +...
Consider the following reaction and calculate the standard Gibbs Free Energy for it. 2 NO + O2 --> 2 NO2 Given that delta H= -114.1 kJ and delta S= -146.5 kJ. Also comment on the spontaneity or otherwise of this reaction at 298 K. Are there any conditions in which your answer might be different? If so state this condition
I have a question about gibbs free energy vs gibbs standard free energy. We know that...
I have a question about gibbs free energy vs gibbs standard free energy. We know that at equilibrium deltaG = 0 and Q = K, and deltaG standard is a non-zero value. But I don't understand. If I want to see if a reaction is at equilibrium then I have to calculate the deltaG standard first, before I can calculate deltaG to see if its value is 0 or not. And everytime I do that, the deltaG standard equals 0...
Using the given data, calculate the change in Gibbs free energy for each of the following...
Using the given data, calculate the change in Gibbs free energy for each of the following reactions. In each case indicate whether the reaction is spontaneous at 298 K under standard conditions. Part A: 2Ag (s) + Cl2 (g) --> 2AgCl (s) Gibbs free energy for AgCl (s) is -109.70 kJ/mol Part B: spontaneous or nonspontaneous Part C: P4O10 (s) + 16H2 (g) --> 4PH3 (g) + 10H2O (g) Gibbs free energy for P4O10 (s) is -2675.2 kJ/mol Gibbs free...
Calculate the standard change in Gibbs free energy, ΔGrxn∘, for the given reaction at 25.0 ∘C....
Calculate the standard change in Gibbs free energy, ΔGrxn∘, for the given reaction at 25.0 ∘C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. KBr(s)↽−−⇀K+(aq)+Br−(aq) ΔGrxn°=    ?    kJ/mol Determine the concentration of K+(aq) if the change in Gibbs free energy, nΔGrxn, for the reaction is −8.95 kJ/mol. [K+] =    ? M
From information in the “Data section” of your textbook, calculate the standard Gibbs free energy and...
From information in the “Data section” of your textbook, calculate the standard Gibbs free energy and the equilibrium constant at (a) 25°C and (b) 50°C for the reaction CH4(g) + 3 Cl2(g) <--> CHCl3(l) + 3 HCl (g). Assume that the reactionenthalpy isindependent of temperature. ΔG°f (CHCl3, l) =-­71.8 kJ/mol, ΔH°f(CHCl3, l) =‐132.2 kJ/mol Which extra DATA can i provide from the textbook. What values should I look for?
verify the maxwell relations associated with the helmholtz free energy F and the Gibbs free energy...
verify the maxwell relations associated with the helmholtz free energy F and the Gibbs free energy F by using the equaiton of state an ideal gas and the expressions for S(T,V) and S(P,V) when cv is constant.
Write a chemical equation for the formation reaction and then calculate the standard free energy of...
Write a chemical equation for the formation reaction and then calculate the standard free energy of formation of each of the following compounds from the enthalpies of formation and the standard molar entropies, using ∆G◦ r = ∆H◦ r - T∆S◦ r: (a) NH3(g) (b) H2O(g) (c) CO(g) (d) NO2(g)
Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn,...
Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T. (Assume that all reactants and products are in their standard states.) Part A ΔH∘rxn=−84kJ, ΔS∘rxn=−157J/K, T=302K Express your answer as an integer. Part B ΔH∘rxn=−84kJ, ΔS∘rxn=−157J/K, T=860K Express your answer as an integer. Part C ΔH∘rxn=84kJ, ΔS∘rxn=−157J/K, T=302K Express your answer as an integer. Part D ΔH∘rxn=−84kJ, ΔS∘rxn=157J/K, T=398K Express your answer as an integer.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT