The enthalpy of fusion, often denoted as $\Delta H_{fus}$, represents the amount of heat required to change a substance from a solid to a liquid at its melting point under constant pressure. It's an endothermic process, meaning heat is absorbed by the substance during the phase transition. Understanding this concept is crucial for various applications, including calorimetry and material science. Let's test your knowledge!
Match the terms with their definitions:
| Term | Definition |
|---|---|
| 1. Enthalpy of Fusion | A. The temperature at which a substance changes from solid to liquid. |
| 2. Melting Point | B. A process that absorbs heat. |
| 3. Endothermic | C. The amount of heat required to melt one mole of a solid at its melting point. |
| 4. Heat Capacity | D. A change of state from liquid to gas. |
| 5. Vaporization | E. The amount of heat required to raise the temperature of a substance by one degree Celsius. |
Complete the following paragraph with the correct terms:
The enthalpy of fusion ($\Delta H_{fus}$) is a measure of the amount of ______ needed to convert a solid into a ______ at its ______ point. This process is considered ______, as it requires the input of energy to overcome the intermolecular forces holding the solid together. A higher enthalpy of fusion indicates ______ intermolecular forces.
Explain, in your own words, how the enthalpy of fusion relates to the strength of intermolecular forces within a substance. Provide an example.
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