At `25^(@)C`, heat evolved due to complete combustion of 7.8 g of `C_(6)H_(6)(l)` is 326.4 kJ. Calculate the heat evolved due to complete combustion of the same amount of `C_(6)H_(6)(l)` at the same temperature and constant pressure of 1 atm.

The heat liberated on complete combustion of 7.8 g benzene is 327 kJ. Calculate heat of combustion measured at constant volume and at 27^@C .

The amount of heat evolved during complete combustion of 7.8 g benzene at constant volume and 27^(@)C is 3270 kJ. Calculate heat of combustion of benzene at constant pressure and 27^(@)C .

At 25^(@)C , the heat of combustion of naphthalene at constant volume is -1230 " kcal mol"^(-1) . Calculate the heat of reaction at constant pressure and 25^(@)C .

At 25^@C at constant volume 7:8 gm benzene produce 326.4 kJ heat on complete combustion, calculate the amount of heat evolved at constant 1 atm pressure and at the temperature on complete combustion of same amount of benzene :

The standard enthalpy of combustion of C_(x)H_(y)(l) at 25^(@)C is Q kJ*mol^(-1) . Write down the thermochemical equation for the combustion reaction of this compound.

Calculate DeltaU and DeltaH in calories if one mole of a monoatomic ideal gas is heated at constant pressure of 1 atm from 25^(@)C to 50^(@)C .

The enthalpy of combustion of C_6H_6(l) is -3250 kJ. When 0.39 g of benzene Is burnt in excess of oxygen in an open vessel, the amount of heat liberated is

At a particular temperature and pressure, the heat produced in the formation of 2 mol of C_(2)H_(6)(g) from the reaction between C_(2)H_(2)(g) and H_(2)(g) is 626 kJ. What amount of H_(2)(g) will react with the required amount of C_(2)H_(2)(g) to produce 939 kJ of heat at the same temperature and pressure?

Calculate the percentage composition of the compound having the molecular formula of C_(6)H_(12)O_(6)(H=1,C=12,O=16) 0.