Electricity required for liberating 710 g of | vedclass

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(B) The electrode reaction for the liberation of chlorine gas is: $2Cl^- \rightarrow Cl_2 + 2e^-$. The molar mass of $Cl_2$ is $71 \ g/mol$. The numbe

Vedclass · Accepted Answer

$1.93 	imes 10^6 \ C$

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(B) The electrode reaction for the liberation of chlorine gas is: $2Cl^- ightarrow Cl_2 + 2e^-$. The molar mass of $Cl_2$ is $71 \ g/mol$. The number of moles of $Cl_2$ liberated is $n = \frac{710 \ g}{71 \ g/mol} = 10 \ mol$. According to the reaction,$1 \ mol$ of $Cl_2$ requires $2 \ mol$ of electrons. Therefore,$10 \ mol$ of $Cl_2$ requires $20 \ mol$ of electrons. The total charge $Q$ required is $Q = n 	imes F = 20 \ mol 	imes 96500 \ C/mol = 1930000 \ C = 1.93 	imes 10^6 \ C$.

Electricity required for liberating $710 \ g$ of $Cl_{2(g)}$ by electrolyzing a concentrated solution of $NaCl$ will be

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