When 1.0g of a compound (molecular weight=28) is burnt in a bomb calorimeter, the temperature of the calorimeter rises from `25^(@)C` to `25.45^(@)C`. Calculate the heat that evolves when 1 mol of this compound is completely burnt `(C_(cal)=2.5kJ*K^(-1))`.

When 1 g of graphite is completely burnt in a bomb calorimeter, the temperature of the bomb and water rises from 25^(@)C to 30.5^(@)C . If the heat capacity of the calorimeter is 5.96kJ*""^(@)C^(-1) , then the heat of combustion per mole of graphite at constant volume is-

When a gas (molar mass =28g*mol^(-1) ) of mass 3.5 is burnt completely in presence of excess oxygen in a bomb calorimeter, the temperature of the calorimeter increases from 298 K to 298.45 K. the heat of combustion at constant volume for the gas (Given: heat capacity of the calorimeter =2.5kJ*K^(-1) ) is-

When 1.0 gm of fructose C_(6) H_(12) O_(6) (s) is burnt in oxygen in a bomb calorimeter, the temperature of the calorimeter water increases by 1.56^(@)C . If the heat capacity of the calorimeter and its contents is 10.0 kJ//^(@)C . Calculate the enthalpy of combustion of fructose at 298 K.

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 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 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 28 was burnt in ress oxygen at 298 K. The temperature of the calorimeter was found to Increase from 298 K to 298.45 K due to the combustion process. Given that the calorimeter constant is 2.5 KJ K^(-1) .Calculate the enthalpy of combustion of the gas in "kJ mol"^(-1) .