Kinetic Theory of Matter and Gas Laws - Chemistry (Undergraduate Foundation)

This course provides a rigorous treatment of the Kinetic Theory and the Gas Laws, explaining the physical principles that control the behaviour of solids, liquids, and gases. We move from the foundational kinetic postulates to the precise mathematical relationships required to model matter's response to energy, pressure, and temperature. These principles dictate real-world engineering, not just textbook theory. You will apply this knowledge to model atmospheric dynamics, design efficient chemical reactors, and optimise engine performance. A command of these laws allows you to quantify substance behaviour under varying conditions, solving the calculation pain points often faced in process engineering and physical science. By the end of this course, you will confidently apply Boyle's, Charles's, Avogadro's, and the Combined Gas Laws to determine unknown state variables. You will derive and utilize the Ideal Gas Equation, PV = nRT, and explain gas properties using kinetic theory postulates. Additionally, you will analyse the structure of solids and calculate gas density. This is a mandatory foundation for Chemistry and Chemical Engineering undergraduates and a prerequisite for thermodynamics. It is intended for learners with a grasp of chemical bonding who require a structured, student-centred alternative to disjointed free resources.

3 hrs

Enrolment valid for 12 months

This course is also part of the following learning track. You may join the track to gain comprehensive knowledge across related courses.

CHM 101: General Chemistry I

This learning track delivers the complete NUC CCMAS curriculum for General Chemistry I. It is a comprehensive programme designed to build a robust, university-level foundation in modern chemistry. The track systematically covers all essential topics, from atomic theory, chemical bonding, and the states of matter, to the quantitative principles of stoichiometry, equilibrium, thermodynamics, and kinetics. This programme is for first-year undergraduates in science, technology, engineering, and mathematics (STEM) faculties who are required to take CHM 101. It is also essential for any student or professional globally who needs a rigorous and complete foundation in first-year university chemistry for further study or career development. This track delivers a full skill set in chemical theory and quantitative problem-solving. Graduates will be able to determine molecular structures, calculate reaction quantities, analyse the energetics and rates of reactions, and solve complex equilibrium problems. This programme provides the non-negotiable prerequisite knowledge for all subsequent chemistry courses and for any degree in the physical sciences, engineering, or medicine.

Course Chapters

1. Introduction

This chapter establishes the course roadmap and introduces the Kinetic Theory of Matter. The theory provides the essential microscopic framework - the motion of particles - required to understand and explain the macroscopic properties and behaviour of gases studied in the following chapters. Upon completion, you will be able to: outline the core postulates of the Kinetic Theory of Matter and appreciate the direct link between particle motion and measurable physical properties like pressure and temperature.

Chapter lessons

1-1. Welcome and postulates

10:33

Welcome to the course; this lesson establishes the course roadmap. We introduce the Kinetic Theory of Matter by defining its core postulates which link the microscopic motion of particles to the macroscopic properties of gases. This theory forms the basis for all subsequent discussions.

2. Kinetic Theory

This chapter systematically applies the Kinetic Theory of Matter to explain the states of matter. We establish how the balance between particle kinetic energy (temperature) and intermolecular forces dictates whether a substance exists as a solid, liquid, or gas, governing phase changes. Upon completion, you will be able to: differentiate the three states of matter based on particle movement, explain the microscopic basis for phase transitions (boiling, melting), and use the kinetic theory to describe the influence of temperature on state.

Chapter lessons

2-1. States of matter

12:08

This lesson differentiates the three primary states of matter - solid, liquid, and gas - based on particle separation and motion. We explain how the strength of intermolecular forces governs a substance's state and its physical properties.

2-2. Temperature and state changes

11:32

This lesson defines phase transitions (melting, boiling, etc.) and the associated thermal changes. We explain how temperature determines whether a substance's kinetic energy is sufficient to overcome intermolecular forces, resulting in a change of state.

3. Gas Laws

This chapter establishes the core empirical laws that describe gas behaviour, starting with the kinetic explanation for pressure. Command of these relationships is essential for accurately calculating unknown state variables and understanding the practical limits of gas systems in engineering and physical science applications. Key objectives include: applying Boyle's, Charles's, Avogadro's, and Gay-Lussac's Laws; deriving and calculating gas density; and mastering the Ideal Gas Equation, PV = nRT, for complex state variable analysis.

Chapter lessons

3-1. Pressure of gases

9:57

This lesson explains the origin of gas pressure using the kinetic theory of matter. We demonstrate how constant, random particle collisions against container walls exert the aggregate force that defines pressure.

3-2. Properties of gases

8:49

This lesson introduces Boyle's Law and Charles's Law, the foundational empirical relationships for gases. We explain the inverse relationship between pressure and volume (Boyle's) and the direct relationship between volume and absolute temperature (Charles's). Master the proportionality and corresponding mathematical forms.

3-3. Calculating density

5:26

This lesson derives the density equation from the Ideal Gas Law. We explain how pressure and temperature affect gas density, and how the molar mass of a gas is directly related to its density. Master this critical derivation for engineering applications.

3-4. Volume laws

13:14

This lesson introduces Avogadro's Law and Gay-Lussac's Law. We establish the direct proportionality between volume and moles, and between pressure and absolute temperature, respectively, under constant conditions. Master these fundamental empirical relationships for solving gas state problems.

4. Conclusion

This final chapter is a mandatory comprehensive assessment designed to confirm full mastery of the course material. Successful completion ensures you can confidently apply both the theoretical principles of the kinetic theory and the practical calculations derived from all gas laws. This is the required preparation for 'Stoichiometry I'. Key objectives include: application of the Ideal Gas Equation and combined gas laws; explaining gas behaviour using kinetic postulates; and validating understanding of the states of matter.

Chapter lessons

4-1. Practice questions

1:32

Apply your knowledge to a comprehensive set of practice questions to confirm mastery of calculations and conceptual explanations. This practice is recommended before commencing 'Stoichiometry I'.