Very small values of Van der Waal's constant in his equation for a particular gas show that:
Correct answer: C. Least attractive forces are present among the molecules of the gas
- A. The molecules of the gas are big sized
- B. Gas is sufficiently polar.
- C. Least attractive forces are present among the molecules of the gas
- D. The gases are non-ideal
Explanation
Very small values of Van der Waal's constant in his equation for a particular gas show that least attractive forces are present among the molecules of the gas.
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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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