What volume of chlorine gas (molar mass 71 g | vedclass

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Question

(A) The electrode reaction for the evolution of chlorine gas is: $2 Cl^{-} \rightarrow Cl_2 + 2 e^{-}$.According to Faraday's law,the number of moles

Vedclass · Accepted Answer

$0.112$

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(A) The electrode reaction for the evolution of chlorine gas is: $2 Cl^{-} ightarrow Cl_2 + 2 e^{-}$.According to Faraday's law,the number of moles of electrons passed is $n(e^{-}) = \frac{I 	imes t}{F} = \frac{1 	imes 965}{96500} = 0.01 \ mol$.From the stoichiometry of the reaction,$2 \ mol$ of $e^{-}$ produce $1 \ mol$ of $Cl_2$.Therefore,moles of $Cl_2$ produced $= \frac{0.01}{2} = 0.005 \ mol$.At $STP$,the volume of $1 \ mol$ of gas is $22.4 \ L$.Volume of $Cl_2 = 0.005 \ mol 	imes 22.4 \ L \ mol^{-1} = 0.112 \ L$.

What volume of chlorine gas (molar mass $71 \ g \ mol^{-1}$) is evolved at $STP$ during electrolysis of fused $NaCl$ by passage of $1 \ A$ current for $965 \ s$ (in $L$)? (At $STP$,$V_m = 22.4 \ dm^3 \ mol^{-1}$)

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