H_{2(g)} + 2 AgCl_{(s)} rightleftharpoons 2 A | vedclass

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(A) For the given reaction,the number of electrons transferred $n = 2$. Given $E^{\circ}_{cell} = 0.22 \ V$ at $25^{\circ} C$. At equilibrium,the rela

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$2.8 	imes 10^{7}$

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(A) For the given reaction,the number of electrons transferred $n = 2$. Given $E^{\circ}_{cell} = 0.22 \ V$ at $25^{\circ} C$. At equilibrium,the relationship between $E^{\circ}_{cell}$ and equilibrium constant $K_{C}$ is given by: $E^{\circ}_{cell} = \frac{0.0591}{n} \log K_{C}$ Substituting the values: $0.22 = \frac{0.0591}{2} \log K_{C}$ $\log K_{C} = \frac{0.22 	imes 2}{0.0591} \approx 7.445$ $K_{C} = 	ext{antilog}(7.445) \approx 2.786 	imes 10^{7} \approx 2.8 	imes 10^{7}$

$H_{2(g)} + 2 AgCl_{(s)} \rightleftharpoons 2 Ag_{(s)} + 2 HCl_{(aq)}$. The $E^{\circ}_{cell}$ at $25^{\circ} C$ for the cell is $0.22 \ V$. The equilibrium constant at $25^{\circ} C$ is

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