Ideal Gas Behavior at High T and Low P

Steps:

• Recall ideal gas law assumes negligible molecular volume and no intermolecular forces.
• Consider real gas deviations: at low T, attractions dominate; at high P, molecular volume matters.
• Evaluate conditions: high T minimizes attractions; low P minimizes volume effects.
• Match to options: B combines both favorable conditions.

Why B is correct:

• High temperature provides kinetic energy to overcome intermolecular forces, while low pressure ensures molecular volume is negligible compared to container volume, aligning with ideal gas assumptions (PV = nRT).

Why the others are wrong:

• A: High pressure causes molecular crowding, amplifying volume deviations.
• C: Low temperature enhances intermolecular attractions, causing non-ideal clustering.
• D: High pressure overrides temperature benefits by increasing molecular interactions.

Final answer: B