Problem: 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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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)


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Problem Details

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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