Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: WBJEE 2019

Given the standard half-cell potentials $\left(\mathrm{E}°\right)$ of the following as

$\mathrm{Zn}⟶{\mathrm{Zn}}^{2+}+2{\mathrm{e}}^{-}; \mathrm{E}°=+0.76 \mathrm{V}$

$\mathrm{Fe}⟶{\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}; \mathrm{E}°=+0.41 \mathrm{V}$

Then the standard e.m.f. of the cell with the reaction ${\mathrm{Fe}}^{2+}+\mathrm{Zn}⟶{\mathrm{Zn}}^{2+}+\mathrm{Fe}$ is

If electrolysis of aqueous ${\mathrm{CuSO}}_4$ solution is carried out using $\mathrm{Cu}$-electrodes, the reaction taking place at the anode is

The charge carried by $1$ millimole of ${\mathrm{M}}^{\mathrm{n}+}$ ions is $193$ coulombs. The value of $\mathrm{n}$ is

What amount of electricity can deposit $1$ mole of Al metal at cathode when passed through molten ${\mathrm{AlCl}}_3$ ?