It's a Hess's law problem. Given the 2 heats of reaction mentioned, you can work out the heat of formation using a Hess's law cycle. (Be careful about stoichiometry.) Your quoted equation doesn't balance. Write Ca + O
2 + 2H
2 Ca(OH)
2 + H
2. The reason for the extra mole of hydrogen will become clear when you set up the Hess's law cycle.
In general, the heat of a reaction can be expressed as Σ ΔH
form(products) - Σ ΔH
form(reactants). But in this case, as all the reactants are pure elements, their heat of formation is zero, so the expression reduces to ΔH
form(Ca(OH)
2) = ΔH
form(Ca(OH)
2).