Exercise-1

The $\mathrm{emf}$ of the cell, $\mathrm{Ni}\left|{\mathrm{Ni}}^{2+}\left(1.0 \mathrm{M}\right)\Vert {\mathrm{Ag}}^{+}\left(1.0 \mathrm{M}\right)\right|\mathrm{Ag}$  [$\mathrm{E}°$  for ${\mathrm{Ni}}^{2+}/\mathrm{Ni}=-0.25$ volt, $\mathrm{E}°$ for ${\mathrm{Ag}}^{+}/\mathrm{Ag}=0.80$ volt] is given by

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left({\mathrm{C}}_1\right)\Vert {\mathrm{Zn}}^{2+}\left({\mathrm{C}}_2\right)\right|\mathrm{Zn}$ for this cell $\mathrm{\Delta G}$ is negative if

Three faradays of electricity was passed through an aqueous solution of iron $\left(\mathrm{II}\right)$ bromide. The mass of iron metal (at. mass $56$) deposited at the cathode is -

A current of $2 \mathrm{A}$ was passed for $1 \mathrm{h}$ through a solution of ${\mathrm{CuSO}}_4. 0.237 \mathrm{g}$ of ${\mathrm{Cu}}^{2+}$ ions were discharged at cathode. The current efficiency is:

A current of $9.65$ $\mathrm{ampere}$is passed through the aqueous solution $\mathrm{NaCl}$ using suitable electrodes for $1000 \mathrm{s}$. The amount of $\mathrm{NaOH}$ formed during electrolysis is:

Which has maximum conductivity:

The ionisation constant of a weak acid electrolyte is $25\times {10}^{-6}$, while the equivalent conductance of its $0.01 \mathrm{M}$ solution is $19.6 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{eq}}^{-1}$. The equivalent conductance of the electrolyte at infinite dilution (in $\mathrm{S} {\mathrm{cm}}^2 {\mathrm{eq}}^{-1}$) will be:

Molar conductances of ${\mathrm{BaCl}}_2, {\mathrm{H}}_2{\mathrm{SO}}_4$ and $\mathrm{HCl}$ at infinite dilutions are ${\mathrm{x}}_1, {\mathrm{x}}_2$ and ${\mathrm{x}}_3$, respectively. Equivalent conductance of ${\mathrm{BaSO}}_4$ at infinite dilution will be: