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Assertion: Real gases behave as ideal ga...

Assertion: Real gases behave as ideal gases most closely at low pressure and high temperature.
Reason: Intermolecular force between ideal gas molecules is assumed to be zero. Choose the appropriate option:
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.

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.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the given question, we need to analyze both the Assertion and the Reason provided. ### Step 1: Analyze the Assertion The assertion states that "Real gases behave as ideal gases most closely at low pressure and high temperature." - **Explanation**: This statement is true. At low pressures, the volume of the gas is large, and the intermolecular forces become negligible compared to the kinetic energy of the gas molecules. At high temperatures, the kinetic energy of the molecules increases, further reducing the effect of intermolecular forces. Therefore, real gases behave more like ideal gases under these conditions. ### Step 2: Analyze the Reason The reason states that "Intermolecular force between ideal gas molecules is assumed to be zero." - **Explanation**: This statement is also true. In the ideal gas model, it is assumed that there are no intermolecular forces acting between the gas molecules. This assumption is what allows the ideal gas law to be applied without considering the interactions between particles. ### Step 3: Determine the Relationship Now we need to determine if the Reason is the correct explanation of the Assertion. - The Assertion is true because real gases behave like ideal gases at low pressure and high temperature due to the dominance of kinetic energy over intermolecular forces. - The Reason is true because ideal gas behavior is based on the assumption of no intermolecular forces. However, while both statements are true, the Reason does not directly explain why real gases behave as ideal gases under the specified conditions. The behavior of real gases at low pressure and high temperature is due to the kinetic energy of the molecules being much larger than the intermolecular forces, rather than the assumption of zero intermolecular forces in ideal gases. ### Conclusion Since both the Assertion and the Reason are true, but the Reason does not correctly explain the Assertion, the correct option is: **b) If both Assertion and Reason are true but Reason is not the correct explanation of Assertion.** ---
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