van der Waal found that tow assumptions made by kinetic thory of gases were wrong. One of them is that gas molecules are

Options

A. Very large
B. Compressible
C. Point particles wihtout significant volume
D. Spherical

Answer

To answer the question regarding the assumptions made by the kinetic theory of gases that Van der Waals found to be incorrect, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Kinetic Theory of Gases**:
- The kinetic theory of gases is based on several assumptions about the behavior of gas molecules. Two of the key assumptions are:
- There are no intermolecular forces between gas molecules.
- The volume of gas molecules is negligible compared to the volume of the container.

2. **Identifying the Incorrect Assumptions**:
- Van der Waals identified that these assumptions do not hold true for real gases.
- Specifically, he pointed out that:
- Gas molecules do exert attractive forces on each other, especially at high pressures and low temperatures.
- The volume occupied by gas molecules is not negligible, and this affects the behavior of gases under certain conditions.

3. **Analyzing the Options**:
- The question asks for one of the assumptions that was found to be wrong. The options provided likely include statements about the nature of gas molecules.
- The third option states that gas molecules are point particles without significant volume, which supports the second assumption that their volume is negligible.

4. **Conclusion**:
- Since Van der Waals showed that the volume of gas molecules cannot be ignored and that they do have attractive forces, the correct answer is that gas molecules are not point particles and their volume is significant.

### Final Answer:
The assumption that gas molecules are point particles without significant volume is incorrect.

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