Apply ΔG° = -nFE°cell to calculate the standard Gibbs energy change from a cell potential, identifying n as the moles of electrons transferred in the balanced equation and using the Faraday constant from the data booklet.
For a different pair of half-cells, the standard Gibbs energy change, , works out to , with a single electron transferred between the electrodes in the cell reaction. Deduce what these two half-cells are. Use…
When the cell discharges, a spontaneous redox reaction generates a potential difference between the electrodes and the temperature of the cell rises. (i) Deduce the signs of , and .…