Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: CG PET 2018

What is the standard potential of the ${\mathrm{Tl}}^{3+}/\mathrm{Tl}$ electrode ?

${\mathrm{Tl}}^{3+}+2{\mathrm{e}}^{-}\to {\mathrm{Tl}}^{+},{\mathrm{E}}^0=1.26\mathrm{V}$

${\mathrm{Tl}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Tl}, {\mathrm{E}}^0=-0.336\mathrm{V}$

Calculate the standard free energy change for the reaction

$2\mathrm{Ag}+2{\mathrm{H}}^{+}\to {\mathrm{H}}_2+2{\mathrm{Ag}}^{+}$ ${\mathrm{E}}^{\circ }$ for ${\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Ag}$ is $0.80 \mathrm{V}$.

The $\mathrm{E}°$ values of the following half cells are given: $\left(25 {}^{\circ }\mathrm{C}\right)$

${\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\to {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+\stackrel{\mathrm{E}°}{0.771 \mathrm{V}}$

${\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\to \mathrm{Fe}\left(\mathrm{s}\right)-0.44 \mathrm{V}$

The $\mathrm{\Delta G}°$ of ${\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{e}}^{-}\to \mathrm{Fe}\left(\mathrm{s}\right)$

Will be, $\left(\mathrm{F}=96485 \mathrm{C} {\mathrm{mol}}^{-1}\right)$

One litre of $1 \mathrm{M} CuS{O}_4$, solution is electrolysed. After passing $2 \mathrm{F}$ charge, the molarity of ${\mathrm{CuSO}}_4$, solution will be:

$2\times {10}^{-5}\mathrm{C}$ charge on ${\mathrm{Zn}}^{2+}$ ions corresponds to

The weight of $\mathrm{Cu}$ deposited, when $2$ Faraday of electricity is passed will be

If $50\times {10}^{-3}$ amp of current is passed through copper coulometer for $60 \min$, calculate the amount of copper deposited $\left(\mathrm{F}=96500 \mathrm{C} {\mathrm{mol}}^{-1}\right)$ (${\mathrm{Cu}}^{+}\to \mathrm{Cu}\left(\mathrm{s}\right)$)

For a fuel cell, which statement is correct?