Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: AMU-AT (B.Tech.) 2019

The emf of the cell Cd $\mid {\mathrm{CdCl}}_2$ (solution) ( $1 \mathrm{atm}$) $\left|\mathrm{AgCl}\right(s\left)\right|\mathrm{Ag}$ is $0.675$ at $25°\mathrm{C}$. The temperature coefficient of the cell is $-65\times {10}^{-4} \mathrm{V} {\mathrm{degree}}^{-1}$ . Find the change in heat content (kJ ${\mathrm{mol}}^{-1}$ ) and entropy $\left(V{\mathrm{deg}}^{-1}\right)$ for the electrochemical reaction that occurs when $1 \mathrm{F}$ of electricity is drawn for it

$0.002\mathrm{M}$ solution of a weak acid has an equivalent conductance $\left(\Lambda \right)60{\mathrm{ohm}}^{-1} {\mathrm{cm}}^2$${\mathrm{eq}}^{-1}$. What will be the $\mathrm{pH}$ ? (Given : $\Lambda °=400{\mathrm{ohm}}^{-1} {\mathrm{cm}}^2{\mathrm{eq}}^{-1}$ ]

The standard emf of the cell $\left({\mathrm{E}}_{\text{cell }}°\right.$ and equilibrium constant $\left({\mathrm{K}}_{\mathrm{eq}}\right)$ of the following reaction of $298 \mathrm{K}$

${\mathrm{Cd}}^{2+}+4{\mathrm{NH}}_3\rightleftharpoons \mathrm{Cd}{\left({\mathrm{NH}}_3\right)}_4^{2+}$

Which colourless gas evolves when ${\mathrm{NH}}_4\mathrm{Cl}$ reacts with zinc in a dry cell battery ?

Ionic mobility of ${\mathrm{Ag}}^{+}$ is $\left({\mathrm{\lambda }}_{{\mathrm{Ag}}^{+}}=5\times {10}^{-1} {\mathrm{ohm}}^{-1} {\mathrm{cm}}^2 {\mathrm{eq}}^{-1}\right)$

The standard e.m.f. of the cell, $\mathrm{Cd}\left(\mathrm{s}\right)\left|{\mathrm{CdCl}}_2\left(\mathrm{aq}\right)\left(0.1\mathrm{M}\right)\right|\left|\mathrm{AgCl}\left(\mathrm{s}\right)\right|\mathrm{Ag}\left(\mathrm{s}\right)$ in which the cell reaction is $\mathrm{Cd}\left(\mathrm{s}\right)+2\mathrm{AgCl}\left(\mathrm{s}\right)⟶2\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cd}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$ is $0.6915 \mathrm{V}$ at $0°\mathrm{C}$ and $0.6753 \mathrm{V}$ at $25°\mathrm{C}$. The enthalpy change of the reaction at $25°\mathrm{C}$ is

The standard e.m.f. for the cell reaction, $2{\mathrm{Cu}}^{+}\left(\mathrm{aq}\right)⟶\mathrm{Cu}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$ is $+0.36 \mathrm{V}$ at $298 \mathrm{K}$. The equilibrium constant of the reaction is