Chemistry - Thermochemistry Question with Solution | TestHub

$2 \mathrm{mol}$of$\mathrm{Hg}\left(\mathrm{g}\right)$is combusted in a fixed volume bomb calorimeter with excess of${\mathrm{O}}_2$at$298 \mathrm{K}$and$1 \mathrm{atm}$into$\mathrm{HgO}\left(\mathrm{s}\right)$. During the reaction, temperature increases from$298.0 \mathrm{K}$to$312.8 \mathrm{K}$. If heat capacity of the bomb calorimeter and enthalpy of formation of$\mathrm{Hg}\left(\mathrm{g}\right)$are$20.00 \mathrm{kJ} {\mathrm{K}}^{-1}$and$61.32 \mathrm{kJ} {\mathrm{mol}}^{-1}$at$298 \mathrm{K}$, respectively, the calculated standard molar enthalpy of formation of$\mathrm{HgO}\left(\mathrm{s}\right)$at$298 \mathrm{K}$is$\mathrm{X} {\mathrm{kJmol}}^{-1}$. The value of$\left|\mathrm{X}\right|$is___[Given: Gas constant$\mathrm{R}=8.3 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$]