Embibe Experts Solutions for Chapter: Electrochemistry, Exercise 4: EXERCISE-III (Analytical Questions)

The reduction potential of hydrogen half-cell will be negative if:

Given are the half-cell reactions : ${\mathrm{Mn}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Mn}; \mathrm{E}°=-1.18 \mathrm{V}; 2({\mathrm{Mn}}^{3+}+2{\mathrm{e}}^{-}\to {\mathrm{Mn}}^{2+}; \mathrm{E}°=+1.51 \mathrm{V}$. The $\mathrm{E}°$ for $3{\mathrm{Mn}}^{2+}\to \mathrm{Mn}+2{\mathrm{Mn}}^{3+ }$will be

The metal that cannot be obtained by electrolysis of an aqueous solution of its salts is?

When, during the electrolysis of a solution of ${\mathrm{AgNO}}_3, 9650$ coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

A current of $9.65\mathrm{A}$ is passed through an aqueous solution of $\mathrm{NaCl}$ using suitable electrodes for $1000 \mathrm{s}$. Given that $1$ faraday equals $96500 \mathrm{C}$ the amount of $\mathrm{NaOH}$ (mol wh. $40.00$ ) formed on electrolysis is:

An electric current is passed through silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed $0.108 \mathrm{g}$ more at the end of the electrolysis. The volume of oxygen evolved at $\mathrm{STP}$ is:

The thermodynamic efficiency of cell is given by

Assertion : Absolute value of ${\mathrm{E}}_{\mathrm{red}}^0$ of an electrode cannot be determined.

Reason : Neither oxidation nor reduction can take place alone.