Question

Standard Reduction (Electrode) Potentials at 25 oC
Half-Cell Reaction	Eo (volts)
Standard Reduction (Electrode) Potentials at 25 oC
Half-Cell Reaction	Eo (volts)
F2(g) + 2 e- 2 F-(aq)	2.87
Ce4+(aq) + e- Ce3+(aq)	1.61
MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l)	1.51
Cl2(g) + 2 e- 2 Cl-(aq)	1.36
Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l)	1.33
O2(g) + 4 H+(aq) + 4 e- 2 H2O(l)	1.229
Br2(l) + 2 e- 2 Br-(aq)	1.08
NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l)	0.96
2 Hg2+(aq) + 2 e- Hg22+(aq)	0.920
Hg2+(aq) + 2 e- Hg(l)	0.855
Ag+(aq) + e- Ag(s)	0.799
Hg22+(aq) + 2 e- 2 Hg(l)	0.789
Fe3+(aq) + e- Fe2+(aq)	0.771
I2(s) + 2 e- 2 I-(aq)	0.535
Fe(CN)63-(aq) + e- Fe(CN)64-(aq)	0.48
Cu2+(aq) + 2 e- Cu(s)	0.337
Cu2+(aq) + e- Cu+(aq)	0.153
S(s) + 2 H+(aq) + 2 e- H2S(aq)	0.14
2 H+(aq) + 2 e- H2(g)	0.0000
Pb2+(aq) + 2 e- Pb(s)	-0.126
Sn2+(aq) + 2 e- Sn(s)	-0.14
Ni2+(aq) + 2 e- Ni(s)	-0.25
Co2+(aq) + 2 e- Co(s)	-0.28
Cd2+(aq) + 2 e- Cd(s)	-0.403
Cr3+(aq) + e- Cr2+(aq)	-0.41
Fe2+(aq) + 2 e- Fe(s)	-0.44
Cr3+(aq) + 3 e- Cr(s)	-0.74
Zn2+(aq) + 2 e- Zn(s)	-0.763
2 H2O(l) + 2 e- H2(g) + 2 OH-(aq)	-0.83
Mn2+(aq) + 2 e- Mn(s)	-1.18
Al3+(aq) + 3 e- Al(s)	-1.66
Mg2+(aq) + 2 e- Mg(s)	-2.37
Na+(aq) + e- Na(s)	-2.714
K+(aq) + e- K(s)	-2.925
Li+(aq) + e- Li(s)	-3.045

Use standard reduction potentials to calculate the equilibrium constant for the reaction:

2Fe³⁺(aq) + Ni(s)2Fe²⁺(aq) + Ni²⁺(aq)

Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.

Equilibrium constant: __________

G° for this reaction would be _________(greater or less) than zero.

Answer 1