Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 1: KCET (UG) 2018

Consider the following electrodes

$\mathrm{P}={\mathrm{Zn}}^{2+}(0.0001\mathrm{M})/\mathrm{Zn} \mathrm{Q}={\mathrm{Zn}}^{2+}(0.1\mathrm{M})/\mathrm{Zn}$

$\mathrm{R}={\mathrm{Zn}}^{2+}(0.01\mathrm{M})/\mathrm{Zn} \mathrm{S}={\mathrm{Zn}}^{2+}(0.001\mathrm{M})/\mathrm{Zn}$

${\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{\mathrm{o}}=-0.76 \mathrm{V}$ electrode potentials of the above electrodes in volts are in the order

In which of the following cases a chemical reaction is possible?

For a cell reaction involving two-electron changes, ${\mathrm{E}}_{\mathrm{cell}}^{\circ }=0.3 \mathrm{V}$ at $25°\mathrm{C}$. The equilibrium constant of the reaction is

${\mathrm{H}}_{2_{\left(\mathrm{g}\right)}}+2{\mathrm{AgCl}}_{\left(\mathrm{s}\right)}\rightleftarrows 2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}+2{\mathrm{HCl}}_{\left(\mathrm{aq}\right)}$

${\mathrm{E}}_{\mathrm{cell}}^{°}$ at $25°\mathrm{C}$ for the cell is $0.22 \mathrm{V}.$ The equilibrium constant at $25°\mathrm{C}$ is

If an aqueous solution of $\mathrm{NaF}$ is electrolyzed between inert electrodes, the product obtained at anode is

The charge required for the reduction of $1$ mole of ${\mathrm{MnO}}_4^{-}$ to ${\mathrm{MnO}}_2$ is

At a particular temperature, the ratio of molar conductance to specific conductance of $0.01 \mathrm{M}$ $\mathrm{NaCl}$ solution is

The resistance of $0.01\mathrm{M} \mathrm{KCl}$ solution at $298 \mathrm{K}$ is $1500 \mathrm{\Omega }.$ If the conductivity of $0.01\mathrm{M} \mathrm{KCl}$ solution at $298 \mathrm{K}$ is $0.1466\times {10}^{-3} \mathrm{S}{ \mathrm{cm}}^{-1}.$ The cell constant of the conductivity cell in ${\mathrm{cm}}^{-1}$ is