If the heats of formation of `C_(2)H_(2)` and `C_(6)H_(6)` are `230 kJ mol^(-1)` and `85 kJ mol^(-1)` respectively, the `DeltaH` value for the trimerisation of `C_(2)H_(2)` is

The enthalpies of formation of C_2H_2(g) and C_6H_6(g) at 298 K are 230 and 85 kJ/mol respectively. The enthalpy change for the reaction 3C_2H_2(g) to C_6H_6(g) is

The standard heats of combustion of CH_(4)(g) and C_(2)H_(6)(g) are -890 kJ*mol^(-1) and -1560 kJ*mol^(-1) , respectively. Why is the calorific value of C_(2)H_(6)(g) lower than that of CH_(4)(g) ?

The molar enthalpies of combustion of C_(2)H_(2)(g), C("graphite") and H_(2)(g) are -1300,-394 , and -286 kJ mol^(-1) , respectively. The standard enthalpy of formation of C_(2)H_(2)(g) is

The molar enthalpies of combustion of C_(2)H_(2)(g), C("graphite") and H_(2)(g) are -1300,-394 , and -286 kJ mol^(-1) , respectively. The standard enthalpy of formation of C_(2)H_(2)(g) is

At 25^(@)C and 1 atm, heat of formation of C_(2)H_(4) (g), CO_(2)(g) and H_(2)O(l) are 52 " kJ mol"^(-1), -394 " kJ mol"^(-1) and -286 " kJ mol"^(-1) respectively. Calculate the heat of combustion of C_(2)H_(4)(g) .

Delta H_("combustion") of C _(6) H _(6) (l) . C(s) and H _(2) (g) are - 3000 kJ ,-390KJ mol^(-1) and - 290 kJ mol ^(-1) respectively. Hence heat of formation of benzene, is

The heats of combustion of C_(2)H_(4), C_(2)H_(6) and H_(2) gases are -1409.5 KJ, -1558.3 KJ and -285.6 KJ respectively. The heat of hydrogenation of ethene is

The heats of combustion of C_(2)H_(4), C_(2)H_(6) and H_(2) gases are -1409.5 KJ, -1558.3 KJ and -285.6 KJ respectively. The heat of hydrogenation of ethene is