(a) (i) Calculate the electrode potential of a half-cell for zinc electrode dipping in 0.01 M ZnSO_4 solution at 25°C. Given: E_Zn^2+ / Zn^o =-0.76 V…

Calculate the electrode potential of a half-cell for zinc electrode dipping in $\displaystyle 0.01$ $\displaystyle \mathrm{M} \mathrm{ZnSO}_{4}$ solution at $\displaystyle 25$°C. Given : $\displaystyle \mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{\mathrm{o}}=-0.76 \mathrm{~V}$ $\displaystyle [\log 10=1]$

Write anode, cathode and overall reaction involved in dry cell.

Equilibrium constant $\displaystyle \left(\mathrm{K}_{\mathrm{c}}\right)$ is related to $\displaystyle \mathrm{E}_{\text {cell }}^{0}$, but not to $\displaystyle \mathrm{E}_{\text {cell }}$. Why ? \[\]

The conductivity of $\displaystyle 0.001$ M solution of acetic acid is $\displaystyle 3.905 \times 10^{-5} \mathrm{~S} \mathrm{~cm}^{-1}$. Calculate its molar conductivity and degree of dissociation ( $\displaystyle \alpha$ ). Given : $\displaystyle \lambda_{\mathrm{CH}_{3} \mathrm{COO}^{-}}^{\mathrm{o}}=40 \cdot 9 \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}$ \[\lambda_{\mathrm{H}^{+}}^{\mathrm{o}}=349 \cdot 6 \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1} \]

Give reasons for the following :

Why does a mercury cell deliver a constant voltage for its entire life ?

Why is it necessary to use salt bridge in a galvanic cell ?