Enthalpies of formation of `CO(g), CO_(2)(g),N_(2)O(g)` and `N_(2)O_(4)(g)` are -110, -393, 81 and 9.7 kJ `mol^(-1)` respectively. Calculate `Delta_(r)H` for the reaction:
`N_(2)O_(4)(g) + 3CO(g) to N_(2)O(g) + 3CO_(2)(g)`.

The enthalpy of formation of CO(g), CO_(2)(g),N_(2)O(g) and N_(2)O_(4)(g) is -110,-393,+81 and 10 kJ / mol respectively. For the reaction N_(2)O_(4)(g)+3CO(g)rarr N_(2)O(g)+3CO_(2)(g). Delta H_(r ) is

The standared enthalpies of formation at 298K for C C1(g), H_(2)O(g), CO_(2)(g) and HC1(g) are -106.7, -241.8, -393.7 , and -92.5kJ mol^(-1) , respectively. Calculate DeltaH^(Theta)underset(298K) for the reaction C C1_(4)(g) +2H_(2)O(g) rarr CO_(2)(g) +4HCI_(g)

Find the value of Delta_(f) H^(@) for the reaction N_(2) O_(4) (g) + 3 CO(g) rarr N_(2) O (g) + 3 CO_(2) (g) Standard enthalpies of formation of CO(g), CI_(2) (g), N_(2) O (g) , and N_(2) O_(4) (g) are - 110, - 393, 81 , and 9.7 kJ mol^(-1) , respectively. Strategy : The standard enthalpy change of a reaction is equal to the sum of the standard molar enthalpie of formation of the products each miltiplied by its stiochiometric coefficient in the balanced equation, minus the corresponding sum of the standard molar enthalpies of formation of the reactants

Delta H_(1)^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -393.5,-110.5 and -241.8 kJ mol^(-1) respectively. Standard enthalpy change for the reacion CO_(2)(g)+H_(2)(g) rarr CO(g) + H_(2)O(g) is