For a Galvanic cell consisting zinc electrode and standard hydrogen electrode,

$$ \mathrm{E}^{\mathrm{o}}\left(\mathrm{Zn}_{(\mathrm{aq})}^{+2} \mid \mathrm{Zn}_{(\mathrm{s})}\right)=-0.76 \mathrm{~V} $$

Identify the reaction that takes place at positive electrode during working of cell?

What is the number of faraday required to form $1 \mathrm{~mol} \mathrm{H}_2$ by reduction of $\mathrm{H}^{+}$ions?

For the cell,

${ }^{\ominus} \mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}^{+2}(1 \mathrm{M})\right|\left|\mathrm{Ag}^{+1}(1 \mathrm{M})\right| \mathrm{Ag}_{(\mathrm{s})}{ }^{\oplus}$

If concentration of $\mathrm{Zn}^{+2}$ decreases to 0.1 M at 298 K , then emf of cell

Calculate the cell constant of conductivity cell containing 0.1 M KCl solution having resistance $60 \Omega$ and conductivity $0.014 \Omega^{-1} \mathrm{~cm}^{-1}$ at $25^{\circ} \mathrm{C}$.