If 3.365 g of ethanol $(l)$ is burnt completely in a bomb calorimeter at 298.15 K , the heat produced is 99.472 kJ . The $\left|\Delta \mathrm{H}_{\mathrm{f}}{ }^{\circ}\right|$ of ethanol at 298.15 K is $\_\_\_\_$ $\times 10^2 \mathrm{~kJ} \mathrm{~mol}^{-1}$. (Nearest integer) Given: Standard enthalpy for combustion of graphite $=-393.5 \mathrm{~kJ} \mathrm{~mol}^{-1}$ Standard enthalpy of formation of water $(\mathrm{l})=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$ Molar mass in $\mathrm{gmol}^{-1}$ of $\mathrm{C}, \mathrm{H}, \mathrm{O}$ are 12,1 and 16 respectively