A.G. Ryder, http://www.nuigalway.ie/chem/AlanR/AryderP20.htm#P20A
2nd year Equilibrium, NUIG: 2007-08, A.G. Ryder
There are 6 topics, each about half a lecture. Each topic builds on the preceding section, to show
how the calculation of equilibrium parameters are fundamental to practical chemistry.
CHEMISTRY TEXTS:
 Atkins’ “Elements of Physical Chemistry” 4th ed.: Chapter 7.
DETAILED COURSE OUTLINE:
Course Topics:
 How does rG vary with composition?
o Basis & Activities.
o Reaction Quotient.
o Equilibrium.
o Equilibrium Constant.
o Spontaneous reactions.
 How does rG vary with composition?
o Basis & Activities…..
o Reaction Quotient.
o Equilibrium.
o Equilibrium Constant.
o Spontaneous reactions.
 Reactions at equilibrium:
o The equilibrium Constant K.
o Calculating K.
o Thermodynamic feasibility.
o Endothermic / Exothermic reactions.
o Effect of temperature.
 The standard reaction Gibbs Energy rG :
o What is it?
o How can it be calculated?
o Standard Gibbs energies of formation.
o Thermodynamic stability.
o Endergonic and Exergonic compounds.
 The equilibrium composition:
o Magnitude of K.
o How to calculate equilibrium concentrations.
o Methodology.
o K in terms of concentration.
o Converting K to Kc.
 Coupled Reactions & response to conditions:
o Coupled reactions.
o Presence of a catalyst.
o Effect of Temperature.
o van’t Hoff Equation.
o Effect of Compression.
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Learning outcomes:
Understand and be able to calculate
reaction quotients and equilibrium
constants. Know how to predict if a
reaction is spontaneous.
Understand and be able to calculate
reaction quotients and equilibrium
constants. Know how to predict whether
or not a reaction is spontaneous.
Know how to calculate K and evaluate if
a reaction is thermodynamically
spontaneous.
Know how to evaluate rG from
thermodynamic data tables.
Know how to calculate equilibrium
concentrations.
Know how to derive van’t Hoff equation.
Evaluate changes in K or composition
with changes in temperature or pressure.