alleryStart learning →Under which conditions does a real gas behave most nearly like an ideal gas?
AHigh pressure and low temperature
BHigh pressure and high temperature
CLow pressure and low temperature
DLow pressure and high temperature
Answer & Solution
Correct answer: D. Low pressure and high temperature
1. The ideal gas equation works when molecular attractions can be ignored and the molecules take up no appreciable share of the volume.
2. Low pressure spreads the molecules far apart, so their own volume is a tiny fraction of the total and attractions barely act.
3. High temperature gives them enough kinetic energy to shrug off whatever attractions remain.
4. Low temperature and high pressure together are the worst case, since crowded slow molecules both attract and take up room.
_Source: OpenStax Chemistry (CC BY 4.0), Ch 9 "Gases", section 9.6 Non-Ideal Gas Behavior_
Keep practising Gases
Browse all Gases questions for IMU CET, or explore more Chemistry topics.
Related questions
The van der Waals equation reduces to PV = nRT under which condition?A 4.25 L flask holds 3.46 mol of carbon dioxide at 229 degrees C. What pressure does the iIn the van der Waals equation, what does the constant b account for?Who developed the first and simplest equation that improves on the ideal gas law?For a gas showing perfectly ideal behaviour, the compressibility factor Z takes which valuKinetic molecular theory explains Boyle's law by which change when the volume of a gas decAt a fixed temperature, how do lighter gas molecules compare with heavier ones?Two different gases are held at the same temperature. What do their molecules share?