1. The dissolving of a particular ionic solid in water, results in a temperature drop of the water. What does this tell us about the relative magnitude of the energy associated with the process of separating the solute particles & separating the solvent particles, and the process of hydrating the ions?

2. If, when 2.00 g of a solid are dissolved completely in 45.3 mL of water in a calorimeter, a temperature rise from 21.5 C to 27.1 C is observed, what is the value of q? (Assume the specific heat capacity of the solution to be the same as that of pure water, 4.184 Jg1C-").

3. The calculation in #2 above does not account for the fact that the calorimeter has a heat capacity = 10.3 J/C. Re-calculate a value for q in #2 above, this time accounting for the energy absorbed by the calorimeter.

4. What must be done to the value of q calculated in #3 above in order to convert delta H value