Define the meaning of the term standard cell potential, $E^\circ_{\text{cell}}$.
The incomplete diagram below shows apparatus that may be used to measure the $E^\circ_{\text{cell}}$ for a cell made from the $\text{Fe}^{3+}/\text{Fe}^{2+}$ and $\text{Ag}^+/\text{Ag}$ half-cells. Finish the diagram and label any components you add.
Identify the substances represented by components A-D.
Use $E^\circ$ values to construct an equation for the cell reaction that occurs if the two electrodes in (a) are joined by a wire and the circuit is completed.
A different electrochemical cell was arranged using $0.31\,\text{mol dm}^{-3}\,\text{Ag}^+(aq)$ rather than the standard Ag solution. Use the Nernst equation, $E = E^\circ + 0.059\log[\text{Ag}^+(aq)]$, and the relevant $E^\circ$ values to calculate the revised $E_{\text{cell}}$ for this experiment.