Kinetic energy of a gas depends upon its

Options

A. Molecules mass
B. Atomic mass
C. Equivalent mass
D. None of these

Explanation

To solve the question regarding what the kinetic energy of a gas depends upon, we can follow these steps:

### Step 1: Understand the Kinetic Theory of Gases
The kinetic theory of gases describes the behavior of gases in terms of particles in motion. According to this theory, the average kinetic energy of gas molecules is directly related to the temperature of the gas.

### Step 2: Identify the Formula for Kinetic Energy
The average kinetic energy (KE) of gas molecules can be expressed with the formula:
\[ KE = \frac{3}{2} RT \]
where:
- \( KE \) is the average kinetic energy,
- \( R \) is the universal gas constant,
- \( T \) is the absolute temperature of the gas in Kelvin.

### Step 3: Analyze the Dependence on Temperature
From the formula, we can see that the kinetic energy is directly proportional to the absolute temperature \( T \). This means:
- As the temperature increases, the kinetic energy increases.
- As the temperature decreases, the kinetic energy decreases.

### Step 4: Consider Other Factors
The question also asks whether the kinetic energy depends on molecular mass, atomic mass, or equivalent mass. According to the formula, these factors do not appear, indicating that they do not affect the kinetic energy of the gas.

### Step 5: Conclusion
Based on the analysis, we conclude that the kinetic energy of a gas depends only on its temperature. Therefore, the correct answer to the question is that it does not depend on molecular mass, atomic mass, or equivalent mass, leading us to select "none of these" as the correct option.

### Final Answer
The kinetic energy of a gas depends only on its temperature.

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