19.6 Cell Potential, Delta G, and the Equilibrium Constant

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ΔG, Ecell, & Keq
ΔG = -nFE
ΔG° = -nFE°
Relates ΔG and Ecell
Relates ΔG° and Ecell°
ΔG° = -RT lnKeq Relates ΔG° and Keq
E°=RT/nF×lnKeq Relates E° and Keq
Spontaneous Reactions
ΔG < 0
Ecell > 0
Q < K

Calculate ΔG° and Kc for the following redox reaction at 298K.
Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq)

REDUCTION POTENTIALS
Al3+ + 3e- → Al -1.66V
Mn2+ + 2e- → Mn -1.18V
Zn2+ + 2e- → Zn -0.76V
Cr3+ + 3e- → Cr -0.74V
Fe2+ + 2e- → Fe -0.44V
Co2+ + 2e- → Co -0.28V
Ni2+ + 2e- → Ni -0.25V
2H+ + 2e- → H2 0V
Cu2+ + 2e- → Cu +0.34V
Ag+ 1e- → Ag +0.80V
Br2 + 2e- → 2Br- +1.07V