\( 2 \) mol of \( \mathrm{Hg(g)} \) is combusted in a fixed volume bomb calorimeter with excess of \( \mathrm{O_2} \) at \( 298 \ \mathrm{K} \) and \( 1 \ \mathrm{atm} \) into \( \mathrm{HgO(s)} \). 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 \( \mathrm{Hg(g)} \) are \( 20.00 \ \mathrm{kJ \ K^{-1}} \) and \( 61.32 \ \mathrm{kJ \ mol^{-1}} \) at \( 298 \ \mathrm{K} \), respectively, the calculated standard molar enthalpy of formation of \( \mathrm{HgO(s)} \) at \( 298 \ \mathrm{K} \) is \( X \ \mathrm{kJ \ mol^{-1}} \). The value of \( |X| \) is _______. \([ \text{Given : Gas constant } R = 8.3 \ \mathrm{J \ K^{-1} \ mol^{-1}} ]\)
