(i) Cu(s) | Cu²⁺ (aq) || Ag⁺ (aq) | Ag(s)
(ii) Cu(s) | Cu²⁺ (aq) || Ag⁺ (aq) | Ag(s)

m = Z x I x t
or          $\mathrm{m}= \frac{108}{96500}\times 0.5\times 2\times 60\times 60$

or           $$\begin{gathered} \mathrm{m}= \frac{108\times 5}{965\times 10}\times 2\times 6\times 6 = 4.03 \mathrm{g} \\ \mathrm{m} = \mathrm{V} \times \mathrm{d} \\ 4.03 = \mathrm{V}\times 10.6 \mathrm{g} {\mathrm{cm}}^{-3} \end{gathered}$$
or                      $$\begin{gathered} \mathrm{V} = \frac{4.03}{10.6 } {\mathrm{cm}}^3 = 0.39 {\mathrm{cm}}^3 \\ \mathrm{V} = \mathrm{area} \times \mathrm{thickness} \end{gathered}$$
or      $0.39 {\mathrm{cm}}^3 = 900 {\mathrm{cm}}^2 \times \mathrm{thickness}$
$\mathrm{Thickness} = \frac{0.39 {\mathrm{cm}}^3}{900 {\mathrm{cm}}^2} = 4.33 \times {10}^{-4} \mathrm{cm}$

(i) Resistance (k) = $3.16 \mathrm{\Omega }$
Conductance (C) = $\frac{1}{\mathrm{R}}$
         = $\frac{1}{3.16 \mathrm{ohm}} = 0.0316 {\mathrm{ohm}}^{-1}$
Specific conductance (k)
                                 = Conductance x cell constant
                                $$\begin{gathered} = 0.0316 {\mathrm{ohm}}^{-1}\times 0.367 {\mathrm{cm}}^{-1} \\ = 0.0116 {\mathrm{ohm}}^{-} {\mathrm{cm}}^{-1} \end{gathered}$$
(ii) Molar conductance (C)
                         $$\begin{gathered} = 0.05 \mathrm{M} = 0.05 \mathrm{mol} {\mathrm{L}}^{-1} \\ = \frac{0.05 \mathrm{mol}}{1 \mathrm{L}} = \frac{0.05 \mathrm{mol}}{{10}^3 {\mathrm{cm}}^3} \\ = 0.05 \times {10}^{-3} \mathrm{mol} {\mathrm{cm}}^{-3} \end{gathered}$$
Molar conductance $\left({\mathrm{\Lambda }}_{\mathrm{m}}\right)$
                          $$\begin{gathered} = \frac{\mathrm{k}}{\mathrm{C}}=\frac{(0.0116 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1})}{(0.05\times {10}^{-3} \mathrm{mol} {\mathrm{cm}}^{-3})} \\ = 232 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}. \end{gathered}$$