Chemistry - Thermodynamics - I Question with Solution | TestHub

${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$ According to thermodynamics's Ist law $$\Delta \mathrm{H}=\Delta \mathrm{E}+\mathrm{nRT}$$ Where $\Delta \mathrm{H}=$ enthalpy of reaction at constant pressure $\Delta \mathrm{E}=$ heat of reaction at constant volume $\mathrm{R}=$ molar gas constant $$\begin{array}{l}\mathrm{T}=\text{ temperature of the reaction }\\ \mathrm{n}=(\text{ no. of moles of product })-(\text{ no. of moles }\end{array}$$ of reactant.) From reaction, $\mathrm{n}={\mathrm{n}}_{\mathrm{p}}-{\mathrm{n}}_{\mathrm{R}}=2-4=-2$ Hence, $\Delta \mathrm{H}=\Delta \mathrm{E}-2\mathrm{RT}$.