5. The decomposition of calcium carbonate to calcium oxide and carbon dioxide only takes place at very high temperatures, making the direct measurement of the enthalpy
change, ∆H for this reaction difficult. Both calcium carbonate and calcium oxide react readily with dilute hydrochloric acid at room temperature.
a) Describe an experiment to find out the enthalpy change of these reactions, describing what you would do and stating what measurement you would make.
b) Which of these two experiments is likely to give the more accurate result? Explain
why?
c) What further piece of data would you need to determine the total energy change in joules associated with the decomposition of calcium carbonate.
d) Given H1 is -110kJ and H2 is -130 kJ determine the H associated with the decomposition of calcium carbonate.

Question

5. The decomposition of calcium carbonate to calcium oxide and carbon dioxide only takes place at very high temperatures, making the direct measurement of the enthalpy
change, ∆H for this reaction difficult. Both calcium carbonate and calcium oxide react readily with dilute hydrochloric acid at room temperature.
a) Describe an experiment to find out the enthalpy change of these reactions, describing what you would do and stating what measurement you would make.
b) Which of these two experiments is likely to give the more accurate result? Explain
why?
c) What further piece of data would you need to determine the total energy change in joules associated with the decomposition of calcium carbonate. 
d) Given H1 is -110kJ and H2 is -130 kJ determine the H associated with the decomposition of calcium carbonate.

anonymous · Answer

$$1. CaO(s) + 2HCl(aq) \rightarrow H2O(l)$$$$2. CaCO3(s) + 2HCl(aq) \rightarrow CaCl2(aq) + H2O(l) + CO2(g)$$


These are the two equations to help with solving the question.

anonymous · Answer

http://en.wikipedia.org/wiki/Hess's_law