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 :

_____is the amount of heat released by a unit weight or unit volume of a fuel during it's complete combustion.

The amount of heat released by a system at constant pressure is 20 kJ. What will be the value of DeltaH in this process?

The amount of heat exchanged with the surrounding at constant temperature and pressure is called

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 .

Calculate heat of combustion of benzene at constant pressure at 27^@C . (R=8.3 J mol^-1 K^-1)

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 .

For an ideal gas, C_(V)=(3)/(2)R . (a) What will be the change in internal energy (DeltaU) of 1 mole of an ideal gas if its temperature is increased by 4K at constant volume ? What would be DeltaU if the temperature of this gas is increased by the same amount of constant pressure? keeping pressure constant if the temperature of that same amount of gas is increased by 4K then what will be the change in internal energy (DeltaU) of that gas? (c) give reason for different values of DeltaU and DeltaH ?

At 25^(@)C , the standard free energy change for a reaction is 5.4 kJ. Calculate the value of equilibrium constant of the reaction at the temperature.

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.

Calculate the enthalpy of combustion of ethylene at 300K at constant pressure if its enthalpy of combustion at constant volume is -"1406 kJ mol"^(-1) .