Under which conditions, does a real gas approximate to an ideal gas?
Correct answer: B. Low Pressure = Low Density = High temp
- A. High Pressure = High Density =High temp
- B. Low Pressure = Low Density = High temp
- C. High Pressure = High Density = Low temp
- D. Low Pressure = Low Density = Low temp
Explanation
A real gas behaves most like an ideal gas at high temperatures and low pressures. High temperatures give molecules enough kinetic energy to overcome intermolecular forces, and low pressures ensure that the volume of the molecules themselves is negligible compared to the total volume.
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About Real and Ideal Gases
An ideal gas is modelled as particles with negligible volume and no intermolecular attraction, obeying Boyle's, Charles's and Avogadro's laws through PV = nRT. Real gases deviate from this behaviour, especially at high pressure and low temperature, because particle volume and attractive forces matter; the van der Waals equation explains these corrections.
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