Question

Charge required for liberating $710g$ of $C{l}_2\left(g\right)$ by electrolyzing a concentrated solution of $NaCl$ will be:

• A. $1.93$ x ${10}^5$ $C$
• B. $1.93$ x ${10}^6$ $C$
• C. $9.65$ x ${10}^6$ $C$
• D. $9.65$ x ${10}^5$ $C$

Answer 1

Answer: (B)

$1.93$ x ${10}^6$ $C$

The reaction taking place at anode is given by:

$2C{l}^{-}\to C{l}_2+2e^{-}$

Thus, $2$ moles of $e^{-}$ are required to liberate $1$ mole of $C{l}_2$

Moles of $C{l}_2=\frac{710}{71}=10$

Hence moles of $e^{-}$ required $=2\times 10=20$

Hence $Q=20F$

$\Rightarrow Q=20\times 96500$

$\Rightarrow Q=1.93\times {10}^{6}C$