We’re being asked to determine the heat (q) absorbed when 347 g of Ca(OH)2 reacts.
The given reaction is:
Ca(OH)2(s) → CaO(s) + H2O(l); ΔH = +65.3kJ
From the balanced equation, we can see that the given ΔH˚rxn (+65.3 kJ) corresponds to 1 mole of Ca(OH)2.
Recall that at constant pressure, heat is equivalent to enthalpy.
q (heat) = ΔH (enthalpy)
How many kilojoules are absorbed when 347 g of Ca(OH)2 reacts?
Ca(OH)2(s) → CaO(s) + H2O(l) ΔH = +65.3kJ
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