Chemical Thermodynamics - Chemistry (Undergraduate Foundation)

This course provides a complete guide to chemical thermodynamics, the study of the energy changes and spontaneity of chemical reactions. It covers the fundamental concepts of enthalpy (heat of reaction), entropy (disorder), and Gibbs free energy. The material details the principles of calorimetry, Hess's law for calculating enthalpy changes, and the use of standard heats of formation. Chemical thermodynamics is essential for predicting the feasibility and energy efficiency of any chemical process. These principles are critical in chemical engineering for designing industrial reactors, in materials science for developing new energy sources and batteries, and in biochemistry for understanding the energy flow that drives metabolic pathways. By the end of this course, you will be able to differentiate between exothermic and endothermic reactions and calculate enthalpy changes using Hess's law and standard heats of formation. You will also be able to use the concepts of entropy and Gibbs free energy to predict whether a chemical reaction will be spontaneous under a given set of conditions. This course is for students who have a solid foundation in chemical equilibria. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of physical chemistry, materials science, and advanced thermodynamics.

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 thermodynamics as the study of energy, heat, work, and spontaneity in chemical reactions. Key learning objectives include: understanding the overall course structure and appreciating the role of thermodynamics in predicting the feasibility of a reaction.

Concept Overviews

1 Lesson

2. Enthalpy

This chapter focuses on enthalpy, the measure of heat change in a chemical reaction. It covers the concepts of exothermic and endothermic reactions and the methods for calculating enthalpy changes. Key learning objectives include: defining enthalpy and standard enthalpy of reaction; and using Hess's Law and standard heats of formation to calculate enthalpy changes.

Concept Overviews

3 Lessons

Problem Walkthroughs

2 Lessons

3. Entropy

This chapter introduces entropy as a measure of disorder or randomness in a system. It covers the second law of thermodynamics and how to predict entropy changes in physical and chemical processes. Key learning objectives include: defining entropy and stating the second law of thermodynamics; and qualitatively predicting whether the entropy change for a given process is positive or negative.

Concept Overviews

2 Lessons

Problem Walkthroughs

1 Lesson

4. Gibbs Free Energy

This chapter introduces Gibbs free energy as the ultimate predictor of reaction spontaneity. It combines the concepts of enthalpy and entropy into a single, decisive thermodynamic function. Key learning objectives include: defining Gibbs free energy (G); using the sign of the change in Gibbs free energy (ΔG) to predict spontaneity; and understanding how temperature affects the spontaneity of a reaction.

Concept Overviews

3 Lessons

Problem Walkthroughs

4 Lessons

5. Conclusion

This concluding chapter summarises the key concepts of chemical thermodynamics. It reinforces the understanding of enthalpy, entropy, and Gibbs free energy as the tools for analysing reaction energetics and spontaneity. This summary prepares the student for the next course, 'Chemical Kinetics', which explores the speed and mechanisms of reactions.

Concept Overviews

2 Lessons