The heat of combustion of carbon is $-394 \mathrm{kJ} {\mathrm{mol}}^{-1}$. The magnitude of heat evolved in the combustion of $6.023\times {10}^{22}$ atoms of carbon is:

If, ${\mathrm{CH}}_3\mathrm{COOH}+{\mathrm{OH}}^{-}\rightleftharpoons {\mathrm{CH}}_3{\mathrm{COO}}^{-}+{\mathrm{H}}_2\mathrm{O}+{\mathrm{Q}}_1$ and ${\mathrm{H}}^{+}+{\mathrm{OH}}^{-}\rightleftharpoons {\mathrm{H}}_2\mathrm{O}+{\mathrm{Q}}_2$, then enthalpy change of the following reaction, ${\mathrm{CH}}_3\mathrm{COOH} \rightleftharpoons {\mathrm{CH}}_3{\mathrm{COO}}^{-}+{\mathrm{H}}^{+}$ is equal to?

For the reaction,

${\mathrm{H}}_2 \left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2 \left(\mathrm{g}\right)\to {\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right), \mathrm{\Delta H}=-285.8 \mathrm{kJ} {\mathrm{mol}}^{-1}$

$\mathrm{\Delta S}=-0.163 \mathrm{kJ} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$.

What is the value of free energy change, at $27 °\mathrm{C}$ for the reaction?