The enthalpies of formation of `N_(2)O` and `NO` are respectively `82` and `90 kJ mol^(-1)`. The enthalpy of reaction
`2N_(2)O(g)+O_(2)(g)to4NO(g)` is

The enthalpies of formation of N_2O and NO at 298 K are 82 and 90 kJ mol^(-1) . The enthalpy of the reaction : 2N_2O_((g)) + 1/2 O_(2(g))rarr 4NO_((g)) is

The enthalpies of formation of N_(2)O and NO at 298 K are 82 and 90 kJ mol^(-1) . The enthalpy of the reaction : N_(2)O(g) + (1)/(2) O_(2) rarr 2 NO(g) is

The enthalpies of formation of N_2O and NO are 28 and 90 kj mol^(-1) respectively. The enthalpy of the reaction, 2N_2O(g)+O_2(g) rarr 4NO(g) is equal to

The enthalpies of formation of N_2O and NO are 28 and 90 kJ mol^-1 respectively. The enthalpy of the reactioin, 2N_2O(g)+O_2(g)rarr4NO(g) is equal to:

The enthapies of formation of N_2O and NO are 28 and 90 kj mol^(-1) respectively. The enthalpy of the reaction, 2N_2O(g)+O_2(g) rarr 4NO(g) is equal to

The enthalpy of formation of N_2O_((g)) and NO_((g)) are 82.0 KJ and 90 KJmol^(-1) respectively. The enthalpy of the reaction 2N_2O_((g)) + O_(2(g)) rarr 4NO_((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 of ammonia is -46.0 kJ mol^(-1) . The enthalpy for the reaction 2N_(2)(g)+6H_(2)(g)to4NH_(3)(g)

The enthalpy of formation of ammonia is -46.0 kJ mol^(-1) . The enthalpy for the reaction 2N_(2)(g)+6H_(2)(g)to4NH_(3)(g)