How long should aqueous NaCl be electrolysed | vedclass

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(C) The electrolysis of aqueous $NaCl$ at the anode involves the oxidation of chloride ions: $2Cl^- (aq) \rightarrow Cl_2 (g) + 2e^-$. From the stoich

Vedclass · Accepted Answer

$965 \ seconds$

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(C) The electrolysis of aqueous $NaCl$ at the anode involves the oxidation of chloride ions: $2Cl^- (aq) ightarrow Cl_2 (g) + 2e^-$. From the stoichiometry,$1 \ mol$ of $Cl_2$ requires $2 \ mol$ of electrons. Therefore,$0.5 \ mol$ of $Cl_2$ requires $0.5 	imes 2 = 1 \ mol$ of electrons. Using Faraday's law,the total charge $Q = n 	imes F$,where $n = 1 \ mol$ and $F = 96500 \ C \ mol^{-1}$. So,$Q = 96500 \ C$. Given current $I = 100 \ A$,we use the formula $Q = I 	imes t$. $t = Q / I = 96500 \ C / 100 \ A = 965 \ seconds$.

How long should aqueous $NaCl$ be electrolysed by passing $100 \ A$ current,so that $0.5 \ mol$ chlorine is released at anode?

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