20. Electrochemistry
Cell Potential: The Nernst Equation
20. Electrochemistry Cell Potential: The Nernst Equation
7PRACTICE PROBLEM
Consider the electrode half-reaction of an alkaline battery:
2 MnO2(s) + H2O(l) + 2 e− → Mn2O3(s) + 2 OH−(aq) E°red = 0.15 V
ZnO(s) + H2O(l) + 2 e− → Zn(s) + 2 OH−(aq) E°red = −1.25 V
How does a fivefold increase in the concentration of NaOH in the electrolyte affect the cell voltage? Explain.
Consider the electrode half-reaction of an alkaline battery:
2 MnO2(s) + H2O(l) + 2 e− → Mn2O3(s) + 2 OH−(aq) E°red = 0.15 V
ZnO(s) + H2O(l) + 2 e− → Zn(s) + 2 OH−(aq) E°red = −1.25 V
How does a fivefold increase in the concentration of NaOH in the electrolyte affect the cell voltage? Explain.