Chemistry - Thermodynamics - II Question with Solution | TestHub

$\Delta {\text{G}}^{\circ }=-{\text{RT ln K}}_{\text{C}}$

$\text{2494.2}=-\text{8.314}\times {\text{300 ln K}}_{\text{C}}$

$\text{2494.2}=-\text{8.314}\times 300\times {\text{2.303 log K}}_{\text{C}}$

$-\frac{\text{2494.2}}{\text{2.303}\times 300\times \text{8.314}}=-\text{0.44}={\text{log K}}_{\text{C}}$

${\text{log K}}_{\text{C}}=-\text{0.44}$

${\text{K}}_{\text{C}}=\text{0.36}$

$\text{Q}=\frac{\left[\mathrm{B}\right]\left[\mathrm{C}\right]}{[\mathrm{A}{]}^2}=\frac{2\times \frac{1}{2}}{{\left(\frac{1}{2}\right)}^2}=4$

$\text{Q}>{\text{K}}_{\text{C}}$, reaction will shift in reverse direction.