Spring Semester

Unit(s) of Assessment	Weighting Towards Module Mark (%)
Examination	80%
Coursework	20%
Qualifying Condition(s)       A weighted aggregate mark of 40% is required to pass the module

This module addresses the essential concepts of chemical thermodynamics that are required by chemical engineers.  Starting from fundamentals, it builds up to prediction of equilibrium states for complex reacting mixtures, and vapour-liquid systems that exhibit non-ideal behaviour.  This will give students an appreciation of what lies beneath chemical engineering flowsheeting and design software packages

Completion of the progress requirements of Level HE1

To provide a solid foundation in Chemical Thermodynamics that will enable interpretation and prediction of a range of chemical and physical transformations such as phase changes and chemical reactions.  This knowledge will underpin and support the associated subjects of reaction engineering and separation processes

Upon successful completion of the module you will be able to:   ·                Recognise the principles whereby process flow-sheeting programmes use chemical thermodynamics to model equilibrium conditions in various unit operations   ·                Demonstrate a sound understanding of the procedures necessary to deduce chemical and phase equilibria from readily available physical property data and state equations, and understand the conventional symbols, reference states and standard conditions used.   ·                Confidently estimate chemical and phase equilibria for ideal and non-ideal systems of moderate complexity over a range of temperatures and pressures and estimate the energy changes involved in changes of chemical composition and physical state.   ·                Accurately evaluate mixture compositions for the various equilibrium systems considered.

Introduction to Chemical Thermodynamics. Symbols and units.   The First Law, Internal energy and Enthalpy.   Thermochemistry, calorimetry, enthalpy of reaction, Hess’s law, Kirchhoff equations   Flame temperature calculation, application of bond energies.   The Second Law of Thermodynamics – concept of entropy   Helmholtz and Gibbs free energies.   Equilibrium for single component phase change Clapeyron, and Clausius-Clapeyron equations   Colligative properties – equilibrium prediction   Chemical Potential and partial molar properties   Gibbs-Duhem equation   Ideal versus non-ideal system behaviour   Non-ideal gas behaviour, equations of state.   Concept of fugacity – determination and calculation   Chemical reaction equilibrium, degree of advancement   Equilibrium constant determination, calculating reaction conversion   Vapour-Liquid equilibrium. Raoult’s law, activity coefficients   Excess Gibbs Free energy, models for predicting VLE

20 hours Lectures, 10 hours Examples classes 2 hour Examination plus 68 hours of independent learning.   Total student learning time 100 hours.

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