AP Chemistry
6.6 Introduction to Enthalpy of Reaction
6.4 Heat Capacity and Calorimetry
6.1 Endothermic and Exothermic Processes
A student uses a coffee-cup calorimeter to determine the molar enthalpy of dissolution of solid potassium nitrate, represented by the equation \(\text{KNO}_3\text{(s)} \rightarrow \text{K}^+\text{(aq)} + \text{NO}_3^-\text{(aq)}\). The student obtains the following data.
Assume that the solution has a specific heat capacity of \(4.00\text{ J/(g}\cdot^\circ\text{C)}\), the calorimeter absorbs negligible heat, and the molar mass of \(\text{KNO}_3\) is \(101\text{ g/mol}\). What is the molar enthalpy of dissolution of \(\text{KNO}_3\text{(s)}\)?
| Measurement | Value |
|---|---|
| Mass of \(\text{KNO}_3\text{(s)}\) | \(10.1\text{ g}\) |
| Mass of water | \(89.9\text{ g}\) |
| Initial temperature | \(25.00^\circ\text{C}\) |
| Final temperature | \(16.25^\circ\text{C}\) |
Assume that the solution has a specific heat capacity of \(4.00\text{ J/(g}\cdot^\circ\text{C)}\), the calorimeter absorbs negligible heat, and the molar mass of \(\text{KNO}_3\) is \(101\text{ g/mol}\). What is the molar enthalpy of dissolution of \(\text{KNO}_3\text{(s)}\)?
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