3 g of ethane undergoes combustion at 27^° C in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by…

$\displaystyle 3$ g of ethane undergoes combustion at $\displaystyle 27^{\circ} \mathrm{C}$ in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by $\displaystyle 0.5$°C. The heat evolved during combustion of ethane at constant pressure is $\displaystyle \_\_\_\_$ $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest integer) [Given : The heat capacity of the calorimeter system is $\displaystyle 20 \mathrm{~kJ} \mathrm{~K}^{-1}, \mathrm{R}=8.3 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$. Assume ideal gas behaviour. Atomic mass of C and H are $\displaystyle 12$ and $\displaystyle 1 \mathrm{~g} \mathrm{~mol}^{-1}$ respectively]