Chemical Thermodynamics - Chemistry (Undergraduate Foundation)

Energy drives every chemical change in our universe. This course explains how heat, work, and internal energy dictate the behaviour of matter from simple phase changes to complex chemical reactions. You will master the laws of thermodynamics, enthalpy calculations, entropy changes, and the ultimate predictor of spontaneity, Gibbs free energy. These principles are the backbone of modern industry. Chemical engineers use them to design efficient industrial reactors and cooling systems. Materials scientists apply them to develop better batteries and energy sources, while biochemists use these same laws to understand the energy flow within living cells. Mastering these concepts is essential for anyone aiming to solve energy-related problems in the real world. By the end of this course, you will be able to distinguish between open, closed, and isolated systems and calculate heat changes using specific heat capacities. You will apply Hess’s law and bond energies to find reaction enthalpies and use the second law of thermodynamics to predict disorder through entropy. Finally, you will calculate Gibbs free energy to determine exactly if and when a reaction will occur naturally under various temperatures. This course is built for undergraduate students in chemistry, chemical engineering, and materials science who need a solid foundation in physical chemistry. It also benefits secondary school leavers preparing for university-level science and professionals looking to refresh their technical knowledge of energy systems. Even those outside these fields will gain a logical framework for understanding how energy and disorder shape the physical world.

6 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

Thermodynamics begins with defining boundaries and energy movement. This chapter teaches you about systems, heat, and work. You need these to track energy in chemical reactions accurately. You will learn to identify system types; explain different forms of work; define specific and molar heat capacities; and calculate heat using mass and temperature changes.

Concept Overviews

4 Lessons

30:39

Problem Walkthroughs

1 Lesson

12:12

2. Enthalpy

Heat tracking is the basis of thermodynamics. This chapter uses enthalpy and the first law to explain how reactions exchange energy with their surroundings. These tools simplify calculations by focusing only on initial and final states. You will learn to calculate internal energy; distinguish exothermic from endothermic reactions; apply standard heats of formation; and use Hess's law to sum intermediate reaction steps.

Concept Overviews

6 Lessons

44:15

Problem Walkthroughs

4 Lessons

25:41

3. Enthalpy of Phase Changes

Substances absorb or release heat when changing state even at a constant temperature. This chapter explains how to quantify these energy shifts during fusion, vaporisation, and sublimation. Mastering these calculations is essential for understanding physical transitions and industrial thermal management. You will learn to define specific enthalpies of phase changes; classify transitions as endothermic or exothermic; calculate molar enthalpy from mass and heat data; and apply Hess's law to relate sublimation to fusion and vaporisation.

Concept Overviews

2 Lessons

10:14

Problem Walkthroughs

2 Lessons

11:15

4. Enthalpy of Reactions

Chemical reactions involve breaking and making bonds, leading to energy shifts known as enthalpy changes. This chapter explains how to measure and calculate these heats of reaction under standard conditions. Understanding these energy balances is vital for predicting reaction behaviour and industrial process efficiency. You will learn to define standard enthalpy changes; distinguish between spontaneous and non-spontaneous processes; calculate reaction heats using bond dissociation energies; and write accurate thermochemical equations from experimental data.

Concept Overviews

3 Lessons

17:17

Problem Walkthroughs

3 Lessons

15:42

5. Entropy

The first law tracks energy but cannot predict if a reaction will occur. This chapter introduces entropy to explain why processes move in specific directions. It is essential for determining reaction spontaneity. You will learn to state the second law of thermodynamics; predict disorder changes from physical states; calculate entropy for phase transitions; and evaluate total entropy using system and surroundings data.

Concept Overviews

4 Lessons

24:56

Problem Walkthroughs

4 Lessons

21:14

6. Gibbs Free Energy

Gibbs free energy is the final way to tell if a reaction will happen on its own. It joins heat and disorder into one value to show spontaneity. This chapter provides the ultimate rules for chemical stability and reaction direction. You will master how to define Gibbs free energy; use its sign to predict if a reaction is spontaneous; explain how temperature changes affect if a reaction occurs; and calculate free energy changes using standard data.

Concept Overviews

4 Lessons

27:24

Problem Walkthroughs

3 Lessons

23:43