Gases are non-ideal at high pressure due to:
Correct answer: C. All of these
- A. Intermolecular forces
- B. Decrease in volume occupied by gas
- C. All of these
- D. Decrease in compressibility of gas
Explanation
Ideal gases are those that have no intermolecular forces, their molecular volume is negligible as compared to the volume of the entire gas and are infinitely compressible.As the pressure on a gas increases, the gas molecules are brought closer together. This decrease in the total volume of the gas brings the molecules so close that intermolecular forces of attraction develop between them. Moreover, the individual volume of a gas molecule is not negligible compared to the now decreased total volume of the gas. Due to the increase in pressure, the gas is already compressed, making further compression more difficult. So, its compressibility decreases.
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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.
Practise Gases
443 free Gases MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
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