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(B) Given: $K_{eq} = 10^{30}$,$T = 298 \ K$.The reaction is $2X_{2(s)} + 3Y^{2+}_{(aq)} 	o 2{X_{2}}^{3+}_{(aq)} + 3Y_{(s)}$.The number of electrons t

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$+0.2955$

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(B) Given: $K_{eq} = 10^{30}$,$T = 298 \ K$.The reaction is $2X_{2(s)} + 3Y^{2+}_{(aq)} 	o 2{X_{2}}^{3+}_{(aq)} + 3Y_{(s)}$.The number of electrons transferred $(n)$ is $6$ (since $X_2$ goes from $0$ to $+3$ oxidation state,$2 	imes 3 = 6$ electrons).The relation between $E^{o}_{cell}$ and $K_{eq}$ is given by $E^{o}_{cell} = \frac{0.0591}{n} \log K_{eq}$.Substituting the values: $E^{o}_{cell} = \frac{0.0591}{6} \log(10^{30})$.$E^{o}_{cell} = \frac{0.0591}{6} 	imes 30$.$E^{o}_{cell} = 0.0591 	imes 5 = 0.2955 \ V$.

The equilibrium constant for the following general reaction is $10^{30}$. Calculate $E^{o}$ for the cell at $298 \ K$ ............ $V$
$2X_{2(s)} + 3Y^{2+}_{(aq)} \to 2{X_{2}}^{3+}_{(aq)} + 3Y_{(s)}$

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The equilibrium constant for the following general reaction is $10^{30}$. Calculate $E^{o}$ for the cell at $298 \ K$ ............ $V$$2X_{2(s)} + 3Y^{2+}_{(aq)} \to 2{X_{2}}^{3+}_{(aq)} + 3Y_{(s)}$