(a) (i) Calculate emf of the following cell at 25°C: Zn ( s )| Zn^2+(0 · 001 M )|| Cd^2+(0 · 1 M )| Cd ( s ) Given: E_Zn^2+ / Zn^o =-0.76 V, E_Cd^2+…

Calculate emf of the following cell at $\displaystyle 25$°C : \[\mathrm{Zn}(\mathrm{~s})\left|\mathrm{Zn}^{2+}(0 \cdot 001 \mathrm{M})\right|\left|\mathrm{Cd}^{2+}(0 \cdot 1 \mathrm{M})\right| \mathrm{Cd}(\mathrm{~s}) \] Given : $\displaystyle \mathrm{E}_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{\mathrm{o}}=-0.76 \mathrm{~V}, \mathrm{E}_{\mathrm{Cd}^{2+} / \mathrm{Cd}}^{\mathrm{o}}=-0.40 \mathrm{~V}[\log 10=1]$

State Faraday's second law of electrolysis. How will the pH of aqueous NaCl solution be affected when it is electrolysed ?

Calculate the $\displaystyle \Delta_{\mathrm{r}} \mathrm{G}^{0}$ and $\displaystyle \log \mathrm{K}_{\mathrm{c}}$ for the following cell reaction : \[\mathrm{Fe}(\mathrm{~s})+\mathrm{Ag}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{Ag}(\mathrm{~s}) \] Given : $\displaystyle \mathrm{E}_{\mathrm{Fe}^{2+} / \mathrm{Fe}}^{\mathrm{o}}=-0.44 \mathrm{~V}, \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathrm{o}}=+0.80 \mathrm{~V}$, \[1 \mathrm{~F}=96500 \mathrm{C} \mathrm{~mol}^{-1} \]

Write any two advantages of the fuel cells over primary and secondary batteries ?

How many Faradays are required for the oxidation of $\displaystyle 1$ mole of $\displaystyle \mathrm{H}_{2} \mathrm{O}$ to $\displaystyle \mathrm{O}_{2}$ ?