Chemical Kinetics - Chemistry (Undergraduate Foundation)

Chemical kinetics determines how fast a reaction occurs and why. This course builds a rigorous foundation in reaction rates, rate laws, integrated kinetics, and the influence of temperature and catalysts on molecular transformations. You will move from basic rate definitions to solving complex problems involving zero, first, and second-order reactions using the Arrhenius equation and experimental data analysis. Understanding reaction kinetics is essential for industrial process control and chemical engineering. Mastery of this subject allows you to predict how changes in concentration, temperature, or the presence of catalysts will impact manufacturing yields, energy consumption, and safety protocols. These principles are the backbone of chemical production, pharmacology, and environmental monitoring, providing the technical basis for optimising output in real-world systems. Upon completion, you will possess the analytical ability to calculate reaction rates, derive rate laws from empirical data, and determine half-life values for various reaction orders. You will be able to apply the collision model to predict reaction behaviour and manipulate the Arrhenius equation to solve for activation energy. These technical skills will enable you to interpret experimental kinetic studies and apply theoretical models to solve practical chemical problems with precision. This course is for undergraduate students building a foundation in chemistry. It is equally valuable for professionals in pharmaceutical, petrochemical, or environmental sectors who require a refresher on kinetic principles to improve efficiency in their daily operations. Even if you are not a chemistry major, the logical framework developed here enhances your quantitative reasoning and problem-solving capabilities, offering a clear advantage in any science or engineering discipline.

4 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 provides the roadmap for the course. It introduces chemical kinetics as the study of the speed of chemical reactions and the factors that influence it. Key learning objectives include: understanding the overall course structure and appreciating the importance of kinetics in controlling chemical processes.

Concept Overviews

1 Lesson

5:00

2. Reaction Rates

This chapter defines reaction rate and its measurement. It provides the essential tools to track how fast reactants turn into products in any chemical system. You will master defining rates; distinguishing average from instantaneous speeds; calculating rates using graph slopes; applying stoichiometric ratios; and using physical or chemical methods to monitor concentration over time.

Concept Overviews

3 Lessons

29:19

3. The Rate Law

This chapter defines the rate law, the mathematical link between reactant concentration and speed. It is essential for predicting and controlling how fast chemical changes occur in any system. You will master writing rate law equations; determining reaction orders using initial rates; applying graphical analysis; and calculating specific rate constants from experimental data.

Concept Overviews

3 Lessons

25:07

Problem Walkthroughs

1 Lesson

9:06

4. Integrated Rate Laws

This chapter explores the direct relationship between reactant concentration and time. You will use integrated rate laws to determine how fast chemicals disappear and predict exactly how much substance remains at any given moment during a reaction. By the end of this section, you will master the integrated rate laws for zero, first, and second-order reactions; identify reaction orders using linear concentration-time graphs; and calculate the half-life for various chemical processes.

Concept Overviews

4 Lessons

28:58

Problem Walkthroughs

5 Lessons

37:30

5. Temperature and Reaction Rate

This chapter explains why reactions speed up as temperature rises. You will master the molecular mechanics of collisions and the energy barriers that control reaction rates, providing the mathematical tools needed to predict chemical behaviour under varying thermal conditions. By the end of this chapter, you will use collision theory to explain reaction speeds, define and identify activation energy on profile diagrams, and apply the Arrhenius equation to calculate rate constants and energy barriers.

Concept Overviews

3 Lessons

17:10

Problem Walkthroughs

2 Lessons

10:02

6. Other Factors

This chapter examines how chemical identity and external agents control reaction speeds. You will learn why some substances react immediately while others require specific conditions or additives to overcome energy barriers. You will master comparing ionic and covalent reaction rates, calculating the impact of surface area on solids, and explaining how catalysts lower activation energy without being consumed.

Concept Overviews

2 Lessons

14:39