Odisha Board Solutions for Chapter: Electrochemistry, Exercise 1: QUESTIONS

${\mathrm{Ag}}^{+} + {\mathrm{e}}^{-} \to \mathrm{Ag} ; {\mathrm{E}}_{\mathrm{cell}}° = +0.8 \mathrm{V}$ and ${\mathrm{Zn}}^{2+} + 2{\mathrm{e}}^{-} \to \mathrm{Zn} ; {\mathrm{E}}_{\mathrm{cell}}° = -0.76 \mathrm{V}$. Calculate the cell potential for the reaction, $2\mathrm{Ag}\left(\mathrm{s}\right) + {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right) \to 2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right) + \mathrm{Zn}\left(\mathrm{aq}\right)$.

Write down the working of mercury dry cell?

Write down the working of nickel cadmium cell.

$\mathrm{E}°$ values for ${\mathrm{Fe}}^{3+}+3{\mathrm{e}}^{-}\to \mathrm{Fe}$ and ${\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Fe}$ are $-0.036 \mathrm{V}$ and $-0.44 \mathrm{V}$ respectively. Calculate $\mathrm{E}°$ and $∆\mathrm{G}°$ for the cell reaction $\mathrm{Fe}+2{\mathrm{Fe}}^{3+}\to 3{\mathrm{Fe}}^{2+}$.
 

When salt spread on road to melt ice and snow during winter, corrosion of motor cars is a major problem, justify.

$\mathrm{E}°$ of $\mathrm{Ag}$ electrode is $0.8 \mathrm{V}$ and solubility product of $\mathrm{AgI}$ is $1\times {10}^{-16}$. Calculate the potential of $\mathrm{Ag}$ electrode at $25 °\mathrm{C}$ in a saturated $\mathrm{AgI}$ solution in water.

State and explain Faraday's laws of electrolysis. How many grams of Aluminium can be produced by the electrolysis of molten alumina with a current of $3$ amperes for $10$ minutes.

Define and explain equivalent conductance and specific conductance. A $0.1 \mathrm{N}$ solution of $\mathrm{NaCl}$ has a specific conductance of $0.00119 \mathrm{mhos} {\mathrm{cm}}^{-1}$. Find its equivalent conductance.