Chemistry - Chemical Equilibrium Question with Solution | TestHub

${\Delta }_{\text{r}}{\text{G}}^{\circ }=0-\text{77.1}\times 2=-\text{154.2 kJ/mol}$

$\text{Q}=\frac{{\left[{\text{H}}^{+}\right]}^2}{{\text{P}}_{{\text{H}}_2}·{\left[{\text{Ag}}^{+}\right]}^2}$

$=\frac{10^{-6}}{\text{0.5}\times \left(10^{-10}\right)}=2\times 10^4$

$\Delta \text{G}={\Delta }_{\text{r}}{\text{G}}^{\circ }+\text{RT ln Q}$

${\Delta }_{\text{r}}\text{G}=-\text{154.2}+\frac{\text{8.314}\times \text{300 ln}\left(2\times 10^4\right)}{1000}$

$=-129.5\; kJ/mol$