1. Which of these gases would behave the least ideally? (O2, N2, and HF)2. Under which conditions would you expect argon to behave ideally? In 150 K, 100 kPaor in 400 K, 100 kPa? Explain.3. Keeping pressure (P) and number of moles (n) constant, what happens to thetemperature (T) if the volume (V) doubles?

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1. Which of these gases would behave the least ideally? (O2, N2, and HF)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 44QRT

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Concept explainers

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.

Question

1. Which of these gases would behave the least ideally? (O2, N2, and HF)
2. Under which conditions would you expect argon to behave ideally? In 150 K, 100 kPa
or in 400 K, 100 kPa? Explain.
3. Keeping pressure (P) and number of moles (n) constant, what happens to the
temperature (T) if the volume (V) doubles?

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