The entropy of vaporisation of benzene is $85 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$. When 117 g of benzene vaporises at its boiling point, what is entropy change of surrounding if process is at equilibrium?

Which from following terms is explained by first law of thermodynamics?

What is the change in internal energy for $2 \mathrm{CO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}$ at $25^{\circ} \mathrm{C}$ ?

( $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \Delta \mathrm{H}=-560 \mathrm{~kJ}$ )