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 3.23 g of CuCl2(s) are dissolved in 100.30 g of water, the temperature of the solution increases from 25.75 to 28.61 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.83 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol

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**Understanding the Heat of Dissolution Using a Coffee Cup Calorimeter**

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

### Experiment Details

In the laboratory, a general chemistry student finds that when **3.23 g of CuCl₂(s)** are dissolved in **100.30 g of water**, the temperature of the solution **increases** from **25.75 to 28.61 °C**.

### Calorimeter Specifications

The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be **1.83 J/°C**.

### Calculation Task

Based on the student's observation, calculate the enthalpy of dissolution of CuCl₂(s) in kJ/mol. 

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

**ΔH_dissolution = [   ] kJ/mol**

This exercise involves applying the principles of calorimetry to determine the heat absorbed or released during the dissolution process.
Transcribed Image Text:**Understanding the Heat of Dissolution Using a Coffee Cup Calorimeter** When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution can be determined using a coffee cup calorimeter. ### Experiment Details In the laboratory, a general chemistry student finds that when **3.23 g of CuCl₂(s)** are dissolved in **100.30 g of water**, the temperature of the solution **increases** from **25.75 to 28.61 °C**. ### Calorimeter Specifications The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be **1.83 J/°C**. ### Calculation Task Based on the student's observation, calculate the enthalpy of dissolution of CuCl₂(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. **ΔH_dissolution = [ ] kJ/mol** This exercise involves applying the principles of calorimetry to determine the heat absorbed or released during the dissolution process.
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