Which of the following gases will be most non-ideal at - 10 deg * C ?
Correct answer: D. SO2
- A. C*O_{2}
- B. N_{2}
- C. H_{2}
- D. SO2
Explanation
Presence of electrons is large in sulphur dioxide and hence greater van der waals interactions . Due to greater intermolecular force it has high boiling point and requires high temperature to behave as ideally. Hence sulphur dioxide behave as least ideal gas at low temperature.
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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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