1. Using the standard reduction potentials listed in Appendix E in the textbook,
ID: 1059428 • Letter: 1
Question
1. Using the standard reduction potentials listed in Appendix E in the textbook, calculate the equilibrium constant for each of the following reactions at 298 K.
A. Fe(s)+Ni2+(aq)?Fe2+(aq)+Ni(s)
B.Co(s)+2H+(aq)?Co2+(aq)+H2(g)
C.10Br?(aq)+2MnO?4(aq)+16H+(aq)?2Mn2+(aq)+8H2O(l)+5Br2(l)
2. If the equilibrium constant for a two-electron redox reaction at 298 K is 1.8×10?4, calculate the corresponding ?G? and E?cel under standard conditions.
2A. Express your answer using two significant figures. Delta G=kJ
2B. Express your answer using two significant figures. E cell= V
Explanation / Answer
1. Equilibrium constant
A. Eo = Ecathode - Eanode
= -0.25 - (-0.44)
= 0.19 V
nFEo = RTlnKeq
2 x 96485 x 0.19 = 8.314 x 298 lnKeq
Keq = 2.67 x 10^6
B. Eo = Ecathode - Eanode
= 0 - (-0.28)
= 0.28 V
nFEo = RTlnKeq
2 x 96485 x 0.28 = 8.314 x 298 lnKeq
Keq = 2.96 x 10^9
C. Eo = Ecathode - Eanode
= 1.51 - 1.066
= 0.444 V
nFEo = RTlnKeq
10 x 96485 x 0.444 = 8.314 x 298 lnKeq
Keq = 1.24 x 10^75
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2. Keq = 1.8 x 10^-4
dGo = -RTlnKeq
= -8.314 x 298 ln(1.8 x 10^-4)
= 21.36 kJ
nFEo = RTlnKeq
2 x 96485 Eo = 21363
Eo = 0.11 V
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