The reaction `3O_(2)(g) rarr 2O_(3)(g), Delta_(r )H > 0`. What can be concluded about average energy per bond in `O_(2)` and `O_(3)`?

The reaction 3O_(2(g)) rarr 2O_(3(g)) is endothermic. What can be concluded about the average per bond in O_(2) and O_(3) ?

The elementary reaction O_3(g) + O(g) rarr 2 O_2(g) is

In the reaction 2H_(2)(g) + O_(2)(g) rarr 2H_(2)O (l), " "Delta H = - xkJ

In the reaction 2H_(2)(g) + O_(2)(g) rarr 2H_(2)O (l), " "Delta H = - xkJ

For the reaction 2H_(2(g)) + o_(2(g)) rarr 2H_(2)O_((g)), Delta H^(@) = - 573.2 kJ . The heat of decomposition of water per mol is:

Consider the reactions (i) S (rhombic) + 3//2O_(2) (g) rarr SO_(3) (g), Delta H_(1) (ii) S (monoclinic) +3//2O_(2) (g) rarr SO_(3) (g), Delta H_(2) (iii) S(rhombic) +O_(3) (g) rarr SO_(3) (g) , Delta H_(3) (iv) S (monoclinic) +O_(3)(g) rarr SO_(3) (g), Delta H_(4) incorrect statement is

From the following data at 25^(@)C {:("Reaction ",Delta_(r) H^(@) kJ//mol),((1)/(2)H_(2)(g) + (1)/(2)O_(2)(g) rarr OH (g),42),(H_(2)(g) + (1)/(2)O_(2)(g) rarr H_(2)O_(g),-242),(H_(2)(g) rarr 2H(g),436),(O_(2)(g) rarr 2O(g),495):} Which of the following statement(s) is/are correct: Statement (a): Delta_(r)H^(@) for the reaction H_(2)O(g) rarr 2H(g) + O(g) Statement (b): Delta_(r)H^(@) for the reaction OH(g) rarr H(g) + O(g) is Statement (c) : Enthalpy of formation of H(g) is -218 kJ/mol Statement (d): Enthalpy of formation of OH(g) is 42 kJ/mol