Study the diagram given below that represents Cu-Ag electrochemical cell and answer the questions…

Study the diagram given below that represents Cu-Ag electrochemical cell and answer the questions that follow. Given $E^\circ_{(\text{Cu}^{2+}/\text{Cu})} = 0\cdot337\text{ V} \text{ ; } E^\circ_{(\text{Ag}^+/\text{Ag})} = 0\cdot799\text{ V}$ (1) Write the cell reaction for the above cell. (2) Calculate the standard emf of the cell. (3) If the concentration of $[\text{Cu}^{2+}]$ is $0\cdot1\text{ M}$ and $E_{\text{cell}}$ is $0\cdot422\text{ V}$, at $25^\circ\text{C}$, calculate the concentration of $[\text{Ag}^+]$. (4) Calculate $\Delta G$ for the cell.

Calculate $\Lambda_m^0$ for $\text{BaCl}_2$ and $\text{Al}_2(\text{SO}_4)_3$ from the following data. For $\Lambda_m^0 \text{ Ba}^{2+} = 127\cdot2\text{ S cm}^2\text{ mol}^{-1}$, $\Lambda_m^0 \text{ Al}^{3+} = 189\text{ S cm}^2\text{ mol}^{-1}$ $\Lambda_m^0 \text{ Cl}^- = 76\cdot3\text{ S cm}^2\text{ mol}^{-1}$, $\Lambda_m^0 \text{ SO}_4^{2-} = 160\text{ S cm}^2\text{ mol}^{-1}$