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 |Δ H_f^°| of ethanol at 298.15 K…

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