# Problem: When a solid dissolves in water, heat may be evolved or absorbed. The  heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when  3.50 g of CuSO4 (s) are dissolved in 115.90 g of water, the temperature of the solution  increases from 24.19 to 27.48°C. The heat capacity of the calorimeter (sometimes referred to as the  calorimeter constant) was determined in a separate experiment to be 1.78 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of  CuSO4 (s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.

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###### FREE Expert Solution
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###### Problem Details

When a solid dissolves in water, heat may be evolved or absorbed. The  heat of dissolution (dissolving) can be determined using a coffee cup calorimeter.

In the laboratory a general chemistry student finds that when  3.50 g of CuSO4 (s) are dissolved in 115.90 g of water, the temperature of the solution  increases from 24.19 to 27.48°C.

The heat capacity of the calorimeter (sometimes referred to as the  calorimeter constant) was determined in a separate experiment to be 1.78 J/°C.

Based on the student's observation, calculate the enthalpy of dissolution of  CuSO4 (s) in kJ/mol.

Assume the specific heat of the solution is equal to the specific heat of water.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Constant-Pressure Calorimetry concept. You can view video lessons to learn Constant-Pressure Calorimetry. Or if you need more Constant-Pressure Calorimetry practice, you can also practice Constant-Pressure Calorimetry practice problems.

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Our tutors rated the difficulty ofWhen a solid dissolves in water, heat may be evolved or abso...as high difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 12 minutes and 7 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Enderle's class at UCD.