Question:
The ideal behaviour of a gas can be achieved best in which of the following conditions?
The ideal behaviour of a gas can be achieved best in which of the following conditions?
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Ideal gas behavior improves at high temperature and low pressure due to negligible intermolecular forces.
Updated On: Jul 18, 2026
- 400 K and 0.01 bar
- 100 K and 0.01 bar
- 400 K and 1 bar
- 100 K and 1 bar
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The Correct Option is A
Solution and Explanation
Step 1: Understand ideal gas conditions.
An ideal gas is best approximated when intermolecular forces are negligible and molecular volume is insignificant. This occurs at high temperature and low pressure conditions.
Step 2: Effect of temperature.
At higher temperature, kinetic energy of gas molecules increases, reducing the effect of intermolecular attractions. Therefore, gases behave more ideally at higher temperatures.
Step 3: Effect of pressure.
At lower pressure, molecules are far apart, and intermolecular interactions become negligible. This improves ideal gas behavior significantly.
Step 4: Analyze given options.
We compare conditions: - 400 K is high temperature - 0.01 bar is very low pressure Thus, this combination best satisfies ideal gas assumptions.
Step 5: Eliminate other options.
100 K is low temperature (less ideal behavior), and 1 bar is relatively higher pressure, both of which increase deviation from ideality. Hence those options are less suitable.
Step 6: Final conclusion.
Therefore, the gas behaves most ideally under: \[ \boxed{400 \, \text{K and } 0.01 \, \text{bar}} \]
An ideal gas is best approximated when intermolecular forces are negligible and molecular volume is insignificant. This occurs at high temperature and low pressure conditions.
Step 2: Effect of temperature.
At higher temperature, kinetic energy of gas molecules increases, reducing the effect of intermolecular attractions. Therefore, gases behave more ideally at higher temperatures.
Step 3: Effect of pressure.
At lower pressure, molecules are far apart, and intermolecular interactions become negligible. This improves ideal gas behavior significantly.
Step 4: Analyze given options.
We compare conditions: - 400 K is high temperature - 0.01 bar is very low pressure Thus, this combination best satisfies ideal gas assumptions.
Step 5: Eliminate other options.
100 K is low temperature (less ideal behavior), and 1 bar is relatively higher pressure, both of which increase deviation from ideality. Hence those options are less suitable.
Step 6: Final conclusion.
Therefore, the gas behaves most ideally under: \[ \boxed{400 \, \text{K and } 0.01 \, \text{bar}} \]
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