Which gas deviates most ideal behavior at room temperature and pressure?
Correct answer: D. Sulphur dioxide
- A. Hydrogen
- B. Nitrogen
- C. Methane
- D. Sulphur dioxide
Explanation
For gas to deviate from ideal behavior, there should be significant intermolecular forces present in the gas. The order of intermolecular forces in gases is: London dispersion forces < Permanent dipole-dipole interactions < Hydrogen bonding.
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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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