Question

During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is__

$2{\mathrm{Cl}}^{-}\to {\mathrm{Cl}}_2+2{\mathrm{e}}^{-}$

• A. $220$ minutes
• B. $330$ minutes
• C. $55$ minutes
• D. $110$minutes

Answer 1

The correct option is D

$110$minutes

The explanation for the correct option:

(D) $110$minutes:

• The chemical reaction is given as

$2{\mathrm{Cl}}^{-}\to {\mathrm{Cl}}_2+2{\mathrm{e}}^{-}$

• According to Faraday's first law of electrolysis:

$$\begin{gathered} \mathrm{w}=\mathrm{Z}\mathrm{x}\mathrm{I}\mathrm{x}\mathrm{t} \\ \mathrm{w}=\frac{\mathrm{E}}{96500}\times \mathrm{I}\times \mathrm{t} \end{gathered}$$

• For $0.1$mole of chlorine, the charge is $2\times 96500\times 0.1$
• Substitute the values in the equation

$\mathrm{t}=\frac{2\times 96500\times 0.10}{3}=6433\mathrm{seconds}=107.33\mathrm{minutes}=110\mathrm{minutes}$

We get,

• $\mathrm{t}=6433.33\mathrm{seconds}=107.33\mathrm{minutes}=110\mathrm{minutes}$

Therefore, option (D) is correct. i.e., during the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is 110 minutes.