The heat of combustion at constant volume at `27^(@)C` of benzene and acetylene are `-800 kcal` and `310 kcal`. Find the heat of polymerisation of acetylene to benzene at constant pressure.

The heat liberated on complete combustion of 7.8 g of benzene at constant volume at 25^(@)C has been found to be 326.39 kJ. Calculate the heat of combustion of benzene at constant pressure.

Explain : Heat of formation of acetylene is +54 kcal.

Given below are some standard heats of reaction (at constant pressure) (A) Heat of formation of water = -68.3 kcal (B) Heat of combustion of acetylene = - 310.6 kcal (C ) Heat of combustion of ethylene = - 337.2 kcal Calculating the heat of reaction for the hydrogenation of acetylene at constant pressure and at constant volume (at 25^(@)C )

The heats of combustion of ethane, ethene and acetylene are -341.1 kcal, -330 kcal and -310.9 kCal mol^(-1) respectively. The best fuel among them is

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 .

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

The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .

The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .

The heat of combusion of benzene in a bomb calorimeter (i.e constant volume) was found to be 3263.9kJ mo1^(-1) at 25^(@)C Calculate the heat of combustion of benzene at constan pressure .