6. Chemical Quantities & Aqueous Reactions
Redox Reactions
6. Chemical Quantities & Aqueous Reactions Redox Reactions
43PRACTICE PROBLEM
A certain voltaic cell uses the half-reactions shown below:
Anode: Zr(s) + 2 H2O(l) → ZrO2(s) + 4 H+(aq) + 4 e–
Cathode: Mn2+(aq) + 2 e– → Mn(s)
Using the thermodynamic values below at 25.0°C, calculate the cell potential (E°) and the equilibrium constant K for the overall cell reaction.
A certain voltaic cell uses the half-reactions shown below:
Anode: Zr(s) + 2 H2O(l) → ZrO2(s) + 4 H+(aq) + 4 e–
Cathode: Mn2+(aq) + 2 e– → Mn(s)
Using the thermodynamic values below at 25.0°C, calculate the cell potential (E°) and the equilibrium constant K for the overall cell reaction.