Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 3: Level 3

The specific conductivity of a saturated solution of $\mathrm{AgCl}$ is $3.40\times {10}^{-6} {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$ at $25°\mathrm{C}$. If ${\mathrm{\lambda }}_{{\mathrm{Ag}}^{+}}=62.3 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1} \& {\mathrm{\lambda }}_{{\mathrm{Cl}}^{-}}=67.7 {\mathrm{ohm}}^{-1} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$, the solubility of $\mathrm{AgCl}$ at $25°\mathrm{C}$ is:

If, $\mathrm{E}{°}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}=-0.440 \mathrm{V}$ and $\mathrm{E}{°}_{{\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}}=0.770 \mathrm{V}$, then $\mathrm{E}{°}_{{\mathrm{Fe}}^{3+}/\mathrm{Fe}}$ is:

The equilibrium constant of a $2$ electron redox reaction at $298 \mathrm{K}$ is $3.8\times {10}^{-3}$. The cell potential $\mathrm{E}°$ (in $\mathrm{V}$) and the free energy change $\mathrm{\Delta G}°$ (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$) for this equilibrium, respectively, are

The density and equivalent weight of a metal are $10.5 \mathrm{g} {\mathrm{cm}}^{-3}$ and $100$, respectively. The time required for a current of $3 \mathrm{amp}$ to deposit a $0.005 \mathrm{mm}$ thick layer of the same metal on an area of $80 {\mathrm{cm}}^2$ is closest to

The specific conductance $\left(\mathrm{K}\right)$ of $0.02 \mathrm{M}$ aqueous acetic acid solution at $298 \mathrm{K}$ is $1.65\times {10}^{-4} \mathrm{S} {\mathrm{cm}}^{-1}$. The degree of dissociation of acetic acid is [Given: equivalent conductance at infinite dilution of ${\mathrm{H}}^{+}=349.1 {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ and ${\mathrm{CH}}_3{\mathrm{COO}}^{-}=40.9 {\mathrm{S}}^2 {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ ].

How much will the potential of a hydrogen electrode change when its solution initially at $\mathrm{pH}=0$ is neutralised to $\mathrm{pH}=7?$

The standard reduction potential of ${\mathrm{Cu}}^{2+}/\mathrm{Cu}$ and ${\mathrm{Cu}}^{2+}/{\mathrm{Cu}}^{+}$ are $0·337$ and $0·153$, respectively. The standard electrode potential of ${\mathrm{Cu}}^{+}/\mathrm{Cu}$ half-cell is:

From the following ${\mathrm{E}}^0$ values of half cells

${\mathrm{A}}^{3-}\to {\mathrm{A}}^{2-}+{\mathrm{e}}^{-}; {\mathrm{E}}^0=1.5 \mathrm{V}$

${\mathrm{B}}^{+}+{\mathrm{e}}^{-}\to \mathrm{B}; {\mathrm{E}}^0=-0.5 \mathrm{V}$

${\mathrm{C}}^{2+}+{\mathrm{e}}^{-}\to {\mathrm{C}}^{+}; {\mathrm{E}}^0=+0.5 \mathrm{V}$

$\mathrm{D}\to {\mathrm{D}}^{2+}+2{\mathrm{e}}^{-}; {\mathrm{E}}^0=-1·5 \mathrm{V}$

What combination of two half cells would result in a cell with the largest potential?