Chemistry - Thermodynamics - II Question with Solution | TestHub

Calculate ${\Delta }_{\mathrm{r}}\mathrm{G}($ in $\mathrm{kJ}/\mathrm{mol})$ for reaction at 300 K

$${\mathrm{N}}_2(\mathrm{g})+{\mathrm{O}}_2(\mathrm{g})\rightleftharpoons 2\mathrm{NO}(\mathrm{g})$$

the partial pressure of ${\mathrm{N}}_2,{\mathrm{O}}_2\&\mathrm{NO}$ are $10^{-4}$ bar, $10^{-2}$ bar and $10^{-5}$ bar respectively when mixed together at 300 K.

Given : 2.303 RT = 5750 J/mol

${\Delta }_{\mathrm{f}}{\mathrm{H}}_{300}^0(\mathrm{NO},\mathrm{g})=90.5\mathrm{kJ}/\mathrm{mol};{\mathrm{S}}_{300}^0\left({\mathrm{N}}_2,\mathrm{g}\right)=190\mathrm{J}/\mathrm{K}-\mathrm{mol}$ ${\mathrm{S}}_{300}^0(\mathrm{NO},\mathrm{g})=210\mathrm{J}/\mathrm{K}-\mathrm{mol};{\mathrm{S}}_{300}^0\left({\mathrm{O}}_2,\mathrm{g}\right)=205\mathrm{J}/\mathrm{K}-\mathrm{mol}$