AP Chemistry
6.6 Introduction to Enthalpy of Reaction
Calcium oxide reacts with water according to the following thermochemical equation:
\[ \text{CaO}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(s) \quad \Delta H^\circ = -64.0 \text{ kJ/mol}_{\text{rxn}} \]
A student adds a \(14.0 \text{ g}\) sample of \(\text{CaO}(s)\) (molar mass \(56.0 \text{ g/mol}\)) to an excess of water at \(25^\circ\text{C}\). What is the enthalpy change, \(\Delta H\), for this process?
\[ \text{CaO}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(s) \quad \Delta H^\circ = -64.0 \text{ kJ/mol}_{\text{rxn}} \]
A student adds a \(14.0 \text{ g}\) sample of \(\text{CaO}(s)\) (molar mass \(56.0 \text{ g/mol}\)) to an excess of water at \(25^\circ\text{C}\). What is the enthalpy change, \(\Delta H\), for this process?
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