Consider two flasks at 25^{$\omicron $}C, one contains an ideal gas and the other contains the real gas SO₃. Which statement regarding these gases is true? A) After the temperature is increased about 100 K, the pressure of the ideal gas will be smaller than the pressure of SO₃ because the van der Waals coefficient a for SO₃ is large. B) As the temperature is decreased, the ideal gas will liquefy first because ideal gases have larger values of the van der Waals coefficient b. C) After the temperature has been lowered about 100 K, the pressure of the ideal gas will be smaller than the pressure of SO₃ because the van der Waals coefficient a for SO₃ is large. D) As the temperature approaches 0 K, the volume of the ideal gas will be larger than the volume of SO₃ because ideal gases lack intermolecular forces. E) As the temperature approaches 0 K, the volume of the ideal gas will be smaller than the volume of SO₃ because ideal gases have larger values of the van der Waals coefficient a.

Question

Quizplus · Accepted Answer

Ideal gases are defined by the lack of intermolecular forces and an infinite capacity to compress, meaning as temperature approaches 0 K, their volume theoretically remains larger than that of real gases, which are affected by intermolecular forces.

Consider Two Flasks at 25 ο\omicron ο C, One Contains an Ideal Gas and the Other Contains

Consider Two Flasks at 25^$\omicron$C, One Contains an Ideal Gas and the Other Contains