At `25^(@)C` the heat of formation of `H_(2)O_((l))` is `-285.9" kJ mole"^(-1)` and that for `H_(2)O_((g))` is `-242.8" kJ mole"^(-1)`. The heat of vaporization of water at the same temperature is

"At 25^(@)C , the standard heat of formation of H_(2)O(l) is -285.83kJ*mol^(-1) "-What does it mean?

The heat of formation of H_(2)O_((l)) is -286.2 kJ. The heat of formation of H_(2)O_((g)) is likely to be

The standard enthalpy of formation of H_(2)O(l) and H_(2)O(g) are -285.8 and -241.8 kJ "mol"^(-1) respectively. What is the heat of vaporisation of water per gram at 25^(@)C and 1 atm?

At 25^(@)C , DeltaG^(@) for the process H_(2)O(l)iffH_(2)O(g) is 8.6 kJ. The vapour pressure of water at this temperature, is nearly :

The heats of formation of CO_(2(g)) and H_(2)O_((l)) are - 398 and -285 kJ mol^(-1) respectively. The heat of combustton of methane is -390 kJ. The heat of formation of methane will be

The enthalpy of the reaction : H_(2)O_(2)(l) rarr H_(2)O(l) + (1)/(2)O_(2)(g) is -98.3 KJ mol^(-1) and the enthalpy of formation of H_(2)O(l) is -285.6 kJ mol^(-1) . The enthalpy of formation of H_(2)O_(2)(l) is :

Heat of formation of H_2 O_((l)), CO_(2(g)) "and" C_2 H_(4(g)) are -285.0, -399.0, and 69.9 kJ/mole respectively. The heat of combustion of ethylene is _________ .

Heat of formation of H_2 O_((l)), CO_(2(g)) "and" C_2 H_(4(g)) are -285.0, -399.0, and 69.9 kJ/mole respectively. The heat of combustion of ethylene is _________ .