0.3 g of ethane undergoes combustion at $27^{\circ} \mathrm{C}$ in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by $0.5^{\circ} \mathrm{C}$. The heat evolved during combustion of ethane at constant pressure is $\_\_\_\_$ $\mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest integer) [Given : The heat capacity of the calorimeter system is $20 \mathrm{~kJ} \mathrm{~K}^{-1}, \mathrm{R}=8.3 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$. Assume ideal gas behaviour. Atomic mass of C and H are 12 and 1 g mol ${ }^1$ respectively]