Given the following standard heats of reactions:
(a) heta of formation of water `= -68.3 kcal`, (b) heat of combustion of `C_(2)H_(2) =- 310.6 kcal`, (c ) heat of combustion of ethylene `=- 337.2 kcal`. Calculate the heat of reaction for the hydrogenation of acetylene at constant volume and at `25^(@)C`.

Given that : (i) heat of formation of water = -68.3 kcal (ii) heat of combustion of acetylene = - 310.6 kcal (iii) heat of combustion of ethylene = - 337.2 kcal. Calculate the heat of reaction for the hydrogenation of acetylene at constant volume (25^(@)C) .

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 heat of formation of CO_(2) and H_(2)O is -97 kcal and -68 kcal. The heat of combustion of benzene is -783 kcal. Calculate the heat of formation of benzene ?

The heat of formation of CO_(2) and H_(2)O is -97 kcal and -68 kcal. The heat of combustion of benzene is -783 kcal. Calculate the heat of formation of benzene ?

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 .