0 . 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 0 . 5 ° C . The heat evolved during combustion of ethane at constant pressure is kJmol - 1 . (Nearest integer) [Given : The heat capacity of the calorimeter system is 20 kJ K - 1 , R = 8 . 3 JK - 1 mol - 1 . Assume ideal gas behaviour. Assume ideal gas behav

Step-by-step solution

The bomb calorimeter is an instrument used to measure the heat of reaction at a fixed volume and the measured heat which is called the change of internal energy. By combustion of 1 mole C 2 H 6 ( ΔU ) = - Heat   capacity × ∆ T mass × Molar   mass = - 20 × 0 . 5 0 . 3 × 30 = - 1000   kJ C 2 H 6 (   g ) + 7 / 2 O 2 (   g ) → 2 CO 2 (   g ) + 3 H 2 O ( l ) Δ ng = 2 - ( 2 + 7 / 2 ) = - ( 7 / 2 ) ΔH = ΔU + ΔnRT = - 1000 - 7 / 2 ×