In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298.0 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is 2.5 kJ K^(-1), find the numerical value for the enthalpy of combustion of the gas in kJ mol^(-1)

In a constant volume calorimeter, 3.5 g of a gas with molecular weight

1.	In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298.0 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is 2.5 kJ K^(-1), find the numerical value for the enthalpy of combustion of the gas in kJ mol^(-1)
Answer» Solution :Heat of combustion of 3.5 G of the gas = Heat TAKEN by the calorimeter= 2.5 (298.45 – 298.0) kJ `9kJ "MOL"^(-1)`