The enthalpies of formation of `CO_(2(g)), H_(2)O_((l))` and `C_(2)H_(4(g))` are respectively `-393.5, -286` and `+52.3 kJ mol^(-1)` the enthalpy change for the combustion of `C_(2)H_(4(g))` is

The enthalpies of formation of CO2(g),H2O(l) and C2H4(g) ​ are respectively −393.5,−286 and +52.3kJmol −1 . The enthalpy change for the combustion of C2H4(g) ​ is ?

The standard enthalpies of formation of H_(2)O(l) and CO_(2)(g) are respectively -286" kJ mol"^(-1) and -394" kJ mol"^(-1) . If the standard heat of combustion of CH_(4)(g)" is "-891" kJ mol"^(-1) , then the standard enthalpy of formation of CH_(4)(g) is

The enthalpy of formation for C_(2)H_(4)(g) , CO_(2)(g) and H_(2)O(l) at 25^(@)C and 1 atm. Pressure be 52 , -394 and -286 kJ mol^(-1) respectively. The enthalpy of combustion of C_(2)H_(4)(g) will be

The standard enthalpies of formation of C_2H_5OH_((l)), CO_(2(g)) and H_2O_((l)) are -277 , -393.5 and -285.5 "kJ mol"^(-1) respectively . Calculate the standard enthalpy change for the reaction C_2H_5OH_((l)) +3O_(2(g)) to 2CO_(2(g)) +3H_2O_((l)) The enthalpy of formation of O_(2(g)) in the standard state is zero , by definition.

If enthalpies of formation of C_(2)H_(4)(g)1 ,CO_(2) and H_(2)O(l) at 25(@)C and 1 atm pressure be 52,-394 and -286kJmol^(-1) respectively ,the enthalpy of combustion of C_(2)H_(4)(g) will be

The enthalpy of formation of C_(2)H_(5)OH(l) , CO_(2)(g) and H_(2)O(l) are - 277.0, -393.5 and -285.5 kJ/mol respectively.Calculate the enthalpy change for the reaction: C_(2)H_(5)OH(l) + 3O_(2)(g) to 2CO_(2)(g) + 3H_(2)O(l) .

If enthalpies of formation of C_(2)H_(4)(g)1 and H_(2)O(l) at 25(@)C and 1 atm pressure be 52,-394 and -286kJmol^(-1) respectively ,the enthalpy of combustion of C_(2)H_(4)(g) will be