During the electrolysis of molten sodium chloride, the time required to produce 0.10 mole of chlorine gas using a current of 3 ampere is

The correct option is A $110minutes$
$NaCl\to N{a}^{-}+C{l}^{-}$
$2C{l}^{-}\to C{l}_{\left(g\right)}+2e^{-}$
By Faradays first lay of electrolysis,
$W=Z\times I\times t$
$W$ is the mass of the substance produced
$\text{W = Moles}\times \text{Molecular mass}$
$I$ is the current in Ampere (A)
$t$ is the time in seconds
$Z$ is the electrochemical equivalent
$W=\frac{E\times I\times t}{F}$

$E=\text{Equivalent mass}$
$t=\frac{W\times F}{E\times I}$

$=\frac{0.1\times 71\times 96500}{35.5\times 3}$

$\approx 110min$