Internal energy is the total energy contained within a thermodynamic system. Calorimetry is the science of measuring the heat associated with chemical reactions or physical changes. In AP Chemistry, you'll often use calorimetry to determine the enthalpy change ($\Delta H$) of a reaction by measuring the heat transferred ($q$) at constant pressure. Key equations include $q = mc\Delta T$ (where $m$ is mass, $c$ is specific heat, and $\Delta T$ is the temperature change) and $\Delta H = q_p$ at constant pressure.
Match the terms with their definitions:
| Term | Definition |
|---|---|
| 1. Enthalpy | A. The energy transferred between objects because of a temperature difference. |
| 2. Heat | B. The study of heat transfer and energy changes in chemical reactions. |
| 3. Calorimetry | C. The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. |
| 4. Specific Heat Capacity | D. The total energy contained within a thermodynamic system. |
| 5. Internal Energy | E. A thermodynamic property that is the sum of the internal energy of the system plus the product of its pressure and volume. |
Answers: 1-E, 2-A, 3-B, 4-C, 5-D
Complete the following paragraph using the words: calorimeter, surroundings, system, temperature, heat.
In thermodynamics, the _________ is the part of the universe we are interested in studying, while the _________ include everything else. A _________ is a device used to measure the amount of _________ absorbed or released during a chemical or physical process. By measuring the change in _________ inside the calorimeter, we can calculate the _________ transferred.
Answers: system, surroundings, calorimeter, heat, temperature, heat
Explain how a coffee-cup calorimeter is used to determine the enthalpy change of a reaction. What assumptions are made in the calculation?
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