Assertion: For a mixture of non reactive ideal gases, the total pressure gets contribution from each gas in the mixture.
Reason: In equilibrium, the average kinetic energy of the molecules of different gases will be equal.

Options

A. If both assertion and reason are true and reason is the correct explanation os assertion.
B. If both assertion and reason are true but reason is not be correct explanation of assertion.
C. If assertion is true but reason is false.
D. If both assertion and reason are false.

Answer

To solve the given question, we need to analyze both the assertion and the reason provided.

### Step 1: Analyze the Assertion
The assertion states: "For a mixture of non-reactive ideal gases, the total pressure gets contribution from each gas in the mixture."

- According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas. This means that each gas contributes to the total pressure based on its own amount (mole fraction) and temperature.
- Therefore, the assertion is **true**.

### Step 2: Analyze the Reason
The reason states: "In equilibrium, the average kinetic energy of the molecules of different gases will be equal."

- The average kinetic energy of gas molecules is given by the formula:
\[ KE_{avg} = \frac{3}{2} k T \]
where \( k \) is the Boltzmann constant and \( T \) is the absolute temperature.
- For ideal gases in thermal equilibrium, the average kinetic energy is dependent on temperature. If different gases are at the same temperature, their average kinetic energies will be equal. However, if they have different degrees of freedom, the average kinetic energy may not be the same.
- For example, a monoatomic gas and a diatomic gas at the same temperature will have different degrees of freedom and thus different average kinetic energies.
- Therefore, the reason is **false**.

### Conclusion
Based on the analysis:
- The assertion is true.
- The reason is false.

Thus, the correct answer is: **Assertion is true, Reason is false.**

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