### Step-by-Step Solution:
1. **Understanding Ideal Gas Behavior**:
- An ideal gas is a theoretical gas that perfectly follows the ideal gas law, which is represented by the equation \( PV = nRT \). In this equation, \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the universal gas constant, and \( T \) is temperature.
2. **Unrestricted Expansion**:
- Unrestricted expansion refers to the process where a gas expands into a vacuum or a larger volume without any external pressure acting against it. In this scenario, the gas does not do any work on the surroundings, and there is no heat exchange with the environment.
3. **Cooling Effect**:
- In real gases, when they expand, they can experience cooling due to intermolecular forces. However, for an ideal gas, there are no intermolecular forces (i.e., the attractions and repulsions between particles are negligible). Therefore, during unrestricted expansion, an ideal gas does not exhibit any cooling effect.
4. **Joule-Thomson Effect**:
- The Joule-Thomson effect describes the temperature change of a real gas when it is allowed to expand freely. For ideal gases, this effect is not applicable because they do not experience any attractive forces that would lead to a temperature change during expansion.
5. **Conclusion**:
- Since the ideal gas does not have any attractive interactions between its molecules, there is no cooling effect during unrestricted expansion. Thus, the correct answer to the question is that there is no cooling effect observed.
### Final Answer:
When an ideal gas undergoes unrestricted expansion, there is no cooling effect observed.
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