Topic C: Gas Laws and Kinetic Molecular Theory
- Page ID
- 169972
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Learning Objectives
WHAT YOU SHOULD BE ABLE TO DO WHEN YOU HAVE FINISHED THIS TOPIC:
- Use classical gas laws to relate changes in pressure, volume, temperature, and number of moles to one another.
- Use vapor pressure information and the classical gas laws to describe the behavior of a gas when it is collected over water.
- Solve stoichiometry problems involving gases, using the ideal gas law.
- Have sufficient understanding of basic kinetic theory to be able to:
- Solve problems involving kinetic energy, temperature, molar mass, and particle velocity for an ideal gas.
- Use effusion rates to determine the molar mass of a gas.
- Answer qualitative questions about the Boltzmann distribution of kinetic energies and velocities, and their relationships to temperature and molar mass.
- Describe the factors that differentiate real gas behavior from the ideal gas model, and use the van der Waals equation to model real gas behavior.
- 5: Gases
- In this chapter, we explore the relationships among pressure, temperature, volume, and the amount of gases. You will learn how to use these relationships to describe the physical behavior of a sample of both a pure gaseous substance and mixtures of gases. By the end of this chapter, your understanding of the gas laws and the model used to explain the behavior of gases.
- 5.1: Characteristics of Gases
- 5.2: Pressure
- 5.3: The Gas Laws
- 5.4: The Ideal Gas Equation
- 5.5: Gas Volumes and Chemical Reactions
- 5.6: Gas Mixtures and Partial Pressures
- 5.7: Kinetic-Molecular Theory
- 5.8: Understanding the Value Distribution of a Variable
- 5.9: Molecular Speed Distribution
- 5.10: Kinetic Energy Distribution
- 5.11: Molecular Effusion and Diffusion
- 5.12: Real Gases - Deviations from Ideal Behavior