If a gas container is placed in a moving train, the temperature of gas will increase.
Kinetic energy of gas molecules will increase.

Options

A. If both Assertion and Reason are true and the reason is correct explanation of the Assertion.
B. If both Assertion and Reason are true but Reason is not the correct explanation of Assertion.
C. If Assertion is true, but the Reason is false.
D. If Assertion is false but the Reason is true.

Explanation

To solve the question regarding the behavior of gas in a container placed in a moving train, we need to analyze both the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Assertion**: The assertion states that the temperature of the gas will increase when the gas container is placed in a moving train.
- **Analysis**: Temperature is a measure of the average kinetic energy of the gas molecules. If the gas molecules are moving randomly, the overall motion of the container (the train moving) does not affect the random motion of the gas molecules inside the container. Therefore, the assertion is **false**.

2. **Understanding the Reason**: The reason states that the kinetic energy of the gas molecules will increase due to the motion of the train.
- **Analysis**: While the gas molecules inside the container are moving randomly, the entire system (the container and the gas) is moving with the train. From an external observer's point of view (like someone standing on the ground), the system has kinetic energy due to its motion. However, the internal kinetic energy of the gas molecules (their random motion) does not change. Thus, the reason is **true** in the context of the system's overall kinetic energy but does not imply a change in the internal kinetic energy of the gas molecules.

3. **Conclusion**: Since the assertion is false and the reason is true, the correct option is that the assertion is false and the reason is true.

### Final Answer:
- Assertion: False
- Reason: True
- Therefore, the correct option is **D**.

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