Calculate standard Gibbs energy for a certain reaction if $\Delta \mathrm{H}^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ respectively are $219 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $-20 \mathrm{JK}^{-1}$.

Calculate the change in internal energy of the system if 15 kJ of work done on the surrounding and system releases 10 kJ of heat in a particular reaction.

For a certain reaction, $\Delta \mathrm{H}^{\circ}=219 \mathrm{~kJ}$ and $\Delta \mathrm{S}^{\circ}=-21 \mathrm{JK}^{-1}$. Find the value of $\Delta \mathrm{G}^{\circ}$.

Calculate the work done in following reaction.

$$ \begin{aligned} & \mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}+\mathrm{HCl}_{(\mathrm{g})} \longrightarrow \mathrm{C}_2 \mathrm{H}_5 \mathrm{Cl}_{(\mathrm{g})} \text { at } 27^{\circ} \mathrm{C} . \\ & \left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right) \end{aligned} $$