19.6 Cell Potential, Delta G, and the Equilibrium Constant
CHECK OUT CHAD'S
PRE-HEALTH PREP
PRE-HEALTH PREP
| ΔG, Ecell, & Keq | |
|---|---|
| ΔG = -nFEΔG° = -nFE° | Relates ΔG and EcellRelates 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 |