The van der waals equation of state for no-ideal gases differs from the ideal gas law in that it accounts for:I) The mass of each molecule of the gas.II) The volume of each molecule of the gas.III) The attractive forces between molecules of the gas
Correct answer: D. II and III only
- A. I, II, and III
- B. I and II only
- C. I and III only
- D. II and III only
Explanation
More significantly, the Van der Waals equation takes into consideration the molecular size and molecular interaction forces (attractive and repulsive forces). Sometimes, it is also referred as the Van der Waals equation of state.
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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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