Write a relation between $∆\mathrm{G}$ and $\mathrm{Q}$ and define the meaning of each term and answer the following :

Explain the effect of an increase in pressure in terms of reaction quotient $\mathrm{Q}$. for the reaction : $\mathrm{CO}\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$ 

We know that the relationship between ${\mathrm{K}}_{\mathrm{c}}$ and ${\mathrm{K}}_{\mathrm{p}}$ is

${\mathrm{K}}_{\mathrm{p}}={\mathrm{K}}_{\mathrm{c}}(\mathrm{RT}{)}^{∆\mathrm{n}}$

What would be the value of $∆\mathrm{n}$ for the given reaction?

${\mathrm{NH}}_4\mathrm{Cl} \left(\mathrm{s}\right) \rightleftharpoons {\mathrm{NH}}_3 \left(\mathrm{g}\right) + \mathrm{HCl} \left(\mathrm{g}\right)$

${\mathrm{PCl}}_5, {\mathrm{PCl}}_3$and ${\mathrm{Cl}}_2$ are at equilibrium at $500\mathrm{K}$ in a closed container and their concentrations are $0.8 \times {10}^{-3} \mathrm{mol} {\mathrm{L}}^{-1}, 1.2 \times {10}^{-3} \mathrm{mol} {\mathrm{L}}^{-1}$ and $1.2 \times {10}^{-3}\mathrm{mol} {\mathrm{L}}^{-1}$respectively.

The value of ${\mathrm{K}}_{\mathrm{c}}$ for the reaction ${\mathrm{PCl}}_5 \left(\mathrm{g}\right) \rightleftharpoons {\mathrm{PCl}}_3 \left(\mathrm{g}\right) + {\mathrm{Cl}}_2 \left(\mathrm{g}\right)$ will be