Physical Chemistry Iii
- Sciences
- 300 level
- 3 credit units
- 180 pages
- 12 units
This course, Physical Chemistry III, is designed for Bachelor of Science chemistry students. It explores thermodynamics, chemical equilibrium, and phase rule concepts. Students will learn about the laws of thermodynamics, fugacity, chemical potentials, and colligative properties. The course also covers reversible and irreversible reactions, entropy changes, and spontaneous processes. Emphasis is placed on understanding the energetics of chemical reactions and applying thermodynamic principles to chemical systems.
About this course
- Difficulty
- Intermediate
- Study hours
- 208 hours
- Maths
- Intermediate
- Content
- Theoretical, problem solving
- Practical work
- No
- Self assessment exercises
- Tutor marked assignments
- Final examination
What you'll read
The real module and unit structure of CHM301, taken from the course material NOUN publishes.
One paragraph, so you can see how it reads
CHM301 · UNIT 2: TYPES OF PROCESSES
Closed system allows exchange of energy (heat or work) with the surroundings but, matter is not allowed to enter or leave it. A properly scaled system (to prevent the passage of matter across its boundary) can be considered as a closed system.
What you should be able to do
- Explain the laws of thermodynamics and their applications.
- Calculate entropy changes in various processes.
- Apply the Gibbs-Helmholtz equation to chemical reactions.
- Determine the spontaneity of a process using thermodynamic criteria.
- Relate fugacity to chemical potentials of an equilibrium system.
What it prepares you for
- Chemical Engineer
- Process Chemist
- Materials Scientist
- Quality Control Analyst
- Petroleum Refining
- Pharmaceuticals
- Chemical Manufacturing
- Environmental Monitoring
Where it gets hard
The units students slow down on, and what makes each one heavy.
- Module 1: Thermodynamics, Types of Process, Heat Change and Enthalpy of Reactions
Unit 4: Enthalpyof Reactions
Application of thermodynamic principles to non-ideal systems requires advanced mathematical skills.
- Module 3: Spontaneous and Non-Spontaneous Processes
Unit 2: Maxwell, Gibbs-Helmholtz and Calusius-Clapeyron Equation
The Gibbs-Helmholtz equation involves partial derivatives and requires a solid understanding of calculus.
A suggested way through it
13 weeks, about 19.5 hours in total. Yours will differ.
- Week 1Module 1: Thermodynamics, Types of Process, Heat Change and Enthalpy of Reactions
Unit 1: Law of Thermodynamic · 1.5 hours
Define system, surroundings, and thermodynamic variables.. Explain the Zeroth Law of Thermodynamics.. Differentiate between extensive and intensive variables..
- Week 2Module 1: Thermodynamics, Types of Process, Heat Change and Enthalpy of Reactions
Unit 2: Types of Processes · 1.5 hours
Define isothermal, adiabatic, and cyclic processes.. Explain work, heat, and heat capacity.. State the First Law of Thermodynamics..
- Week 3Module 1: Thermodynamics, Types of Process, Heat Change and Enthalpy of Reactions
Unit 3: Heat Change · 1.5 hours
Explain internal energy of a system.. Calculate work done on an ideal gas in isothermal processes.. State the significance of enthalpy and enthalpy change of a system..
- Week 4Module 1: Thermodynamics, Types of Process, Heat Change and Enthalpy of Reactions
Unit 4: Enthalpyof Reactions · 1.5 hours
Explain Joule-Thomson Effect.. Derive Kirchhoff's Equation and state its significance.. Define bond enthalpy and calculate enthalpies of reactions from bond enthalpies..
- Week 5Module 2: Reversible and Irreversible Reactions, Entropy of Change
Unit 1: Reversible, Irreversible and Cyclic Process · 1.5 hours
Differentiate between reversible and irreversible processes based on heat exchange.. Describe Carnot cycle and derive an expression for the efficiency of a Carnot engine..
- Week 6Module 2: Reversible and Irreversible Reactions, Entropy of Change
Unit 2: Entropy of Change · 1.5 hours
Define entropy.. State the Second Law of Thermodynamics.. Calculate entropy changes for isothermal and non-isothermal processes..
- Week 7Module 2: Reversible and Irreversible Reactions, Entropy of Change
Unit 3: Entropy of Mixing · 1.5 hours
Derive an expression for calculating entropy of mixing.. Calculate entropy changes in phase transitions and chemical reactions..
- Week 8Module 3: Spontaneous and Non-Spontaneous Processes
Unit 1: Free energy functions · 1.5 hours
Distinguish between spontaneous and non-spontaneous processes.. Define Helmholtz free energy and Gibbs free energy.. Calculate ∆A and ∆G for different processes..
- Week 9Module 3: Spontaneous and Non-Spontaneous Processes
Unit 2: Maxwell, Gibbs-Helmholtz and Calusius-Clapeyron Equation · 1.5 hours
Derive Maxwell relations.. Derive Gibbs-Helmholtz equation.. Explain the significance of Clausius-Clapeyron equation..
- Week 10Module 3: Spontaneous and Non-Spontaneous Processes
Unit 3: Criteria for Spontaneity · 1.5 hours
Explain the criteria for spontaneity.. State and explain the Third Law of Thermodynamics..
- Week 11Module 4: Colligative Properties
Unit 1: System of Various Comparison · 1.5 hours
Define partial molar quantities.. Define fugacity.. Identify the components of an ideal gas..
- Week 12Module 4: Colligative Properties
Unit 2: Derivation of General Expression for Chemical Equilibrium · 1.5 hours
Explain the chemical equilibrium constant.. Identify expressions for an ideal gas mixture.. Correlate between equilibrium constant and concentration..
- Week 13Module 4: Colligative Properties
Unit 3: Thermodynamic Quantities from EMF Values · 1.5 hours
State the colligative properties.. Define phase rule and component.. Explain the term configuration..
Preparing for the exam
- Review and understand all the laws of thermodynamics, focusing on their mathematical expressions and practical applications.
- Practice solving numerical problems related to entropy, enthalpy, and Gibbs free energy calculations from TMAs and examples.
- Create concept maps linking Maxwell's relations, Gibbs-Helmholtz equation, and Clausius-Clapeyron equation to understand their interdependencies.
- Focus on understanding the conditions for spontaneity and how they relate to different thermodynamic potentials.
- Memorize key formulas and equations, and practice applying them to different scenarios.
- Pay close attention to units and conversions in calculations to avoid errors.
- Review all self-assessment exercises and tutor-marked assignments (TMAs) to identify areas of weakness and focus your study efforts.
Questions students ask about this course
What is CHM301 about?
This course, Physical Chemistry III, is designed for Bachelor of Science chemistry students. It explores thermodynamics, chemical equilibrium, and phase rule concepts. Students will learn about the laws of thermodynamics, fugacity, chemical potentials, and colligative properties. The course also covers reversible and irreversible reactions, entropy changes, and spontaneous processes. Emphasis is placed on understanding the energetics of chemical reactions and applying thermodynamic principles to chemical systems.
How many units does CHM301 have?
CHM301, Physical Chemistry Iii, has 12 units across 4 modules, over 180 pages of course material. You can read it one unit at a time.
How many credit units is CHM301?
CHM301 carries 3 credit units, at 300 level in Sciences.
Is CHM301 hard?
CHM301 is rated intermediate level, with intermediate mathematical content. It is mostly theoretical and problem solving work.
How long does CHM301 take to study?
About 208 hours of study, spread across its 12 units.
How is CHM301 assessed?
CHM301 is assessed by self assessment exercises, tutor marked assignments and final examination.
What can I do with CHM301?
Chemical Engineer, Process Chemist, Materials Scientist and Quality Control Analyst.