Heat of combustion of ethanol to give `CO_2` and water at constant pressure and `27^@C is `327 kcal. How much heat is evolved in (cal) in combustion at constant volume at `27^@C`?

The heat of combustion of ethanol into carbon dioxide and water is –327 kcal at constant pressure. The heat evolved (in cal) at constant volume and 27^(@)C (if all gases behave ideally) is (R = 2 cal mol^(–1) K^(–1) __________.

The heat of combustion of ethylene at 18^(@)C and at constant volume is -330.0 kcal when water is obtained in liquid state. Calculate the heat of combustion at constant pressure and at 18^(@)C ?

The heat of combustion of ethylene at 18^(@)C and at constant volume is -335.8 kcal when water is obtained in liquid state. Calculate the heat of combusion at constant pressure and at 18^@C .

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 ?

For a reaction 2A(g)+2B(g) rarr 2C(g)+D(g) . If heat of reaction at constant pressure is -28 K.cal. The heat of reaction at constant volume at 27^(@)C is

The heat liberated on complete combustion of 7.8g benzene is 327kJ . This heat has been 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))

For combustion of 1 mole of benzene at 25^(@)C , the heat of reaction at constant pressure is -780.9" kcal." What will be the heat of reaction at constant volume ? C_(6)H_(6(l))+7(1)/(2)O_(2(g))rarr 6CO_(2(g))+3H_(2)O_((l))