Electrochemistry

Give the chemical equation that represents the reduction of liquid water ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ at the platinum anode.

How is molar conductivity of an aqueous solution of an electrolyte measured experimentally?

Explain with a suitable example the relation between the Gibbs energy of chemical reaction (G) and the functioning of the electrochemical cell.

State and explain the Nernst equation with the help of a metallic electrode and anon-metallic electrode.

Explain the variation of molar conductivity with the change in concentration of the electrolyte. Give reasons.

What are the products obtained at cathode and the anode during the electrolysis of the following when platinum electrodes are used in the electrolysis?

Aqueous ${\mathrm{K}}_2{\mathrm{SO}}_4$ solution

What are the products obtained at cathode and the anode during the electrolysis of the following when platinum electrodes are used in the electrolysis?

Aqueous ${\mathrm{CuSO}}_4$ solution

On what factors the electrical conductance of an aqueous electrolyte solution depends?

What are fuel cells? How are they different from galvanic cells? Give the construction of ${\mathrm{H}}_2, {\mathrm{O}}_2$ fuel cell.

What is metallic corrosion? Explain it with respect to iron corrosion?

What are primary and secondary batteries? Give one example of each.

What are the products obtained at cathode and the anode during the electrolysis of the following when platinum electrodes are used in the electrolysis.

Molten $\mathrm{KCl}$

What is electrolysis? Give Faraday's first law of electrolysis?

State and explain kohlrausch's law of independent migration of ions.

Give the construction and working of a standard hydrogen electrode with a neat diagram.

What are galvanic cells? Explain the working of a galvanic cell with a neat sketch taking Daniel cell as example.

Calculate the degree of dissociation $\left(\mathrm{\alpha }\right)$ of ${\mathrm{CH}}_3\mathrm{COOH}$ at $298\mathrm{K}$. Given that

$$\begin{gathered} {{\mathrm{\Lambda }}^{\mathrm{m}}}_{{\mathrm{CH}}_3\mathrm{COOH}} = 11.75 {\mathrm{cm}}^2 {\mathrm{mol}}^{-1} \\ {\mathrm{\Lambda }}_{{\mathrm{CH}}_3{\mathrm{COO}}^{-}}^{\mathrm{o}} = 40.95 {\mathrm{cm}}^2 {\mathrm{mol}}^{-1} \\ {\mathrm{\Lambda }}_{{\mathrm{H}}^{+}}^{\mathrm{o}} = 349.15 {\mathrm{cm}}^2 {\mathrm{mol}}^{-1} \end{gathered}$$

The conductivity of $0.20\mathrm{M}$ solution of $\mathrm{KCl}$ at $298\mathrm{K}$ is $0.0248 \mathrm{S} {\mathrm{cm}}^{-1}$. Calculate molar conductance.

$$\begin{gathered} {\mathrm{Cu}}^{2+} + 2{\mathrm{e}}^{-} \rightleftharpoons \mathrm{Cu} ; {\mathrm{E}}^{\mathrm{o}} = +0.34\mathrm{V} \\ {\mathrm{Ag}}^{+} + {\mathrm{e}}^{-} \rightleftharpoons \mathrm{Ag} ; {\mathrm{E}}^{\mathrm{o}} = +0.80\mathrm{V} \end{gathered}$$

For what concentration of ${\mathrm{Ag}}^{+}$ ions will be the emf of the cell be zero at 25^oC. The concentration of ${\mathrm{Cu}}^{2+}$ is $0.1\mathrm{M}$. $\left(\log 3.919 =0.593 \right)$

Calculate the emf of the cell with the cell reaction

 $\mathrm{Ni} + 2{\mathrm{Ag}}^{+} \left(0.002\mathrm{M}\right) \to {\mathrm{Ni}}^{2+}\left(0.160\mathrm{M}\right) + 2\mathrm{Ag}; {\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}} = 1.05\mathrm{V}$