If the Delta G^o for the cell reaction AgCl_{ | vedclass

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(C) The given reaction is: $AgCl_{(s)} + \frac{1}{2} H_{2(g)} \rightarrow Ag_{(s)} + H^+ + Cl^-$,with $\Delta G^o_1 = -21.52 \, kJ$. The target reacti

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$-43.04$

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(C) The given reaction is: $AgCl_{(s)} + \frac{1}{2} H_{2(g)} ightarrow Ag_{(s)} + H^+ + Cl^-$,with $\Delta G^o_1 = -21.52 \, kJ$. The target reaction is: $2AgCl_{(s)} + H_{2(g)} ightarrow 2Ag_{(s)} + 2H^+ + 2Cl^-$. This target reaction is exactly twice the first reaction. Since $\Delta G^o$ is an extensive property,multiplying the stoichiometric coefficients by a factor of $2$ results in the $\Delta G^o$ value being multiplied by the same factor. Therefore,$\Delta G^o_2 = 2 	imes \Delta G^o_1 = 2 	imes (-21.52 \, kJ) = -43.04 \, kJ$.

$A$. Leclanche cell	$1$. Converts energy of combustion into electrical energy
$B$. Fuel cell	$2$. Rechargeable cell
$C$. Ni-Cd cell	$3$. At anode,$Zn \longrightarrow Zn^{2+} + 2e^{-}$

If the $\Delta G^o$ for the cell reaction $AgCl_{(s)} + \frac{1}{2} H_{2(g)} \rightarrow Ag_{(s)} + H^+ + Cl^-$ is $-21.52 \, kJ$,what will be the $\Delta G^o$ for the reaction $2AgCl_{(s)} + H_{2(g)} \rightarrow 2Ag_{(s)} + 2H^+ + 2Cl^-$ (in $, kJ$)?

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Pick out the incorrect statement $:-$

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