(a(i))[1]
Define the term standard cell potential, $E^\circ_{\text{cell}}$.
(a(ii))[1]
Complete the diagram, and label the parts you add.
(a(iii))[3]
Identify the components A-D.
(b(i))[1]
Use $E^\circ$ values to write an equation for the cell reaction that occurs when the two electrodes in (a) are linked by a wire and the circuit is completed.
(b(ii))[2]
A different electrochemical cell was assembled with $0.31\,\text{mol dm}^{-3}\,\text{Ag}^+(aq)$ rather than the standard Ag solution. Apply the Nernst equation, $E = E^\circ + 0.059\log[\text{Ag}^+(aq)]$, together with the appropriate $E^\circ$ values to determine the new $E_{\text{cell}}$ for this experiment.