For the reaction : $2 \mathrm{NO}_{2(\mathrm{~g})} \rightarrow \mathrm{N}_{2} \mathrm{O}_{4(\mathrm{

Question

For the reaction : $2 \mathrm{NO}_{2(\mathrm{~g})} ightarrow \mathrm{N}_{2} \mathrm{O}_{4(\mathrm{~g})}$, when $\Delta S=176.0 \mathrm{~J} \mathrm{~K}^{-1}$ and $\Delta H=-57.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the magnitude of $\Delta G$ at 298 K for the reaction is $\qquad$ $\mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest integer)\

Professor PC Thomas Classes · Answer

(5) : $2 \mathrm{NO}_{2(g)} ightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4(g)}$\ $\Delta G=\Delta H-T \Delta S$\ $=-57.8-\left(-176 	imes 298 	imes 10^{-3}ight.$\ $=-57.8 \mathrm{~kJ} / \mathrm{mol}+52.448 \mathrm{~kJ} / \mathrm{mol}$\ $=-5.35 \mathrm{~kJ} / \mathrm{mol}$\