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- If the heat of dissolution of anhydrous <img alt="\mathrm{\mathrm{CuSO}_4 \: and \: \mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}\: is -60 \mathrm{KJ} / \mathrm{mol} \: and -11.2 \mathrm{KJ} / \m
If the heat of dissolution of anhydrous respectively, then heat of hydration
to form
is
71.2
-71.2
48.8
-48.8
Answers (1)
Let's consider the following reaction:
The heat of dissolution of , which means that when 1 mole of
dissolves in water,
of heat is released.
The heat of dissolution of , which means that when 1 mole of
dissolves in water,
of heat is released.
Now, let's consider the hydration of . This can be represented as follows:
We can break this reaction into two steps:
1. Hydration of
2. Dissolution of in excess water:
The heat of hydration of can be calculated by subtracting the enthalpy change of the second step from the enthalpy change of the overall reaction:
where is the enthalpy change of the hydration step and
is the enthalpy change of the dissolution step.
Since is formed,
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