of copper (II) sulfate
You are provided with :
The aim of this activity is to measure the enthalpy of hydration of copper sulfate using Hess's Law .
|The enthalpy of hydration is difficult to calculate as it is not possible to measure the chemical potential energy directly as the CuSO4.5H2O crystallizes.|
We can calculate the ΔH of equation 3 if we know the ΔH of equation 1 and 2.
You will perform this practical in two stages.
Then you will use a calorimeter to measure the ΔH of equation 2.
Using Hess's Law you will then work out the ΔH of equation 3.
This has two parts.
Part one - reverse equation 1
Part two - add it to equation 2.
|Step 1 measure the mass of a crucible|
|Step 2 Measure accurately about 23.0 g of copper sulfate pentahydrate (CuSO4.5H2O )|
|Step 3 Add 100 mL of distilled water to the calorimeter|
|Step 4 Measure the temperature of the water.|
|Step 5 Add the CuSO4.5H2O to the water and seal the calorimeter. Stir the the water to allow for the CuSO4.5H2O to dissolve.|
|Step 6 Record the final temperature of the water.|
Step 7 Calculate the ΔH. of the reaction below
CuSO4 .5H2O (s) + (aq) => CuSO4(aq) + H2O(l)