Chemistry - Thermodynamics - II Question with Solution | TestHub

Combustion of Hydrogen in a fuel cell at$\text{300}\text{K}$is represented as$\text{2}{\text{H}}_{\text{2}}\left(\text{g}\right)\text{+}{\text{O}}_{\text{2}}\left(\text{g}\right)\to \text{2}{\text{H}}_{\text{2}}\text{O}\left(\text{g}\right)$. If$\mathrm{\Delta }\mathrm{H}$and$\mathrm{\Delta }\mathrm{G}$are$-\text{241}{\text{.80 kJ mol}}^{-\text{1}}$and$-228.60{\text{ kJ mol}}^{-1}$respectively for${\mathrm{H}}_2\mathrm{O}$then the value of$\mathrm{\Delta }\mathrm{S}$for the above process is: