ThermochemistryHard

Question

Formation of ozone from oxygen is an endothermic process. In the upper atmosphere, ultraviolet is the source of energy that drives the reaction. Assuming that both the reactions and the products of the reaction are in standard states, the standard enthalpy of formation of ozone from the following information

3O2(g) → 2O3(g), ΔHo = 286 kJ, is

Options

A.+143 kJ/mol
B.−143 kJ/mol
C.+286 kJ/mol
D.−286 kJ/mol

Solution

$\Delta_{f}H_{O_{3}(g)} = - \frac{286}{2} = 143\text{ kJ/mol}$

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