. 2.3 g of an organic compound of molecular mass 46 is subjected to combustion in presence of excess of oxygen in a constant volume calorimeter the thermal capacity of which is 2.0 kJ/K. In case the temperature of the calorimeter increases from 27°c to 27.225°C in the combustion process, find the heat of combustion at constant volume of the compound in kJ.

The heat of combustion of H_(2)(g) at constant pressure and 300k is -280kJ mol^(-1) . What will be the heat of combustion at constant volume and at 300K ?

In a constant volume calorimeter 5g of a gas with molecular weight 40 was burnt in excess of oxygen at 298 K.the temperature of the calorimeter was found to increase from 298 K to 298.75 K due to combustion process.Given that the heat capacity of the calorimeter is 2.5 kJ K^(-1),a numerical value for the DeltaU of combustion of the gas in kJ mol^(-1) is

0.5 g of benzoic acid was subjected to combustion in a bomb calorimeter at 15^(@)C when the temperature of the calorimeter system (including water) was found to rise by 0.55^(@)C . Calculate the heat of combustion of benzoic acid (i) at constant volume and (ii) at constant pressure. the thermal capacity of the calorimeter including water was found to be 23.85 kJ.

A 1.250 g sample of octane (C_(8)H_(18)) is burned in excess of oxygen in a bomb calorimeter. The temperature of calorimeter rises from 294.05 K to 300.78 K . If heat capacity of the calorimeter is 8.93 kJ K^(-1) , find the heat transferred to calorimeter.

When 2 g of benzene are burnt in a bomb calorimeter, the heat produced is 83.6 kJ at 298 K. Calculate the enthalpy of combustion of benzene.

The heat of combustion of solid benzoic acid at constant volume is -321.30 kJ at 27^(@)C . The heat of combustion at constant pressure is

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)

The heat of combustion of solid benzoic acid at constant volume is -321.3 kJ at 27 degree Celcius . The heat of combustion at constant pressure is

When 1.0 g of oxalic acid (H_(2)C_(2)O_(4)) is burnt in a bomb calorimeter whose capacity is 8.75 KJ/K, the temperature increases by 0.312K, the enthalpy of combustion of oxalic acid at 27^(@)C is :