Question

The liberation of $1$ mole of chlorine requires how many Faradays of electricity?

• A. $0.5$ Faraday
• B. $0.25$ Faraday
• C. $2$ Faradays
• D. $4$ Faradays

Answer 1

The correct option is C $2$ Faradays

$2C{l}^{-}\to C{l}_2+2e^{-}$
$Q=n\left(e^{-}\right)\times F$
2mol electrons are liberated in production of 1mol of chlorine.
therefore electricity required for the process
$\Rightarrow$ $=2\times F$ = $2$ Faradays