Question:
A gas behaves more closely as an ideal gas at
A gas behaves more closely as an ideal gas at
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Think "Far and Fast": molecules need to be far apart (low pressure) and moving fast (high temperature) to ignore each other.
Updated On: Jul 4, 2026
- Low pressure and low temperature
- Low pressure and high temperature
- High pressure and low temperature
- High pressure and high temperature
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The Correct Option is B
Solution and Explanation
Step 1: Concept
Real gases deviate from ideal behavior due to intermolecular forces and the finite volume of gas molecules.
Step 2: Meaning
Ideal behavior assumes negligible molecular volume and no attractive forces between molecules.
Step 3: Analysis
At high temperatures, molecules have high kinetic energy to overcome attractive forces. At low pressures, molecules are far apart, making their individual volumes negligible compared to the total volume.
Step 4: Conclusion
Therefore, the combination of low pressure and high temperature minimizes deviations, making a real gas behave like an ideal gas. Final Answer: (B)
Real gases deviate from ideal behavior due to intermolecular forces and the finite volume of gas molecules.
Step 2: Meaning
Ideal behavior assumes negligible molecular volume and no attractive forces between molecules.
Step 3: Analysis
At high temperatures, molecules have high kinetic energy to overcome attractive forces. At low pressures, molecules are far apart, making their individual volumes negligible compared to the total volume.
Step 4: Conclusion
Therefore, the combination of low pressure and high temperature minimizes deviations, making a real gas behave like an ideal gas. Final Answer: (B)
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