Equilibrium
Learning outcomes - after studying this topic, you should be able to:
- explain chemical equilibrium as a reaction mixture whose composition is unchanging in time, and relate this to the kinetic picture of equal rates of formation and decomposition of reactants and products
- define the equilibrium constant, and write it down for an arbitrary gas phase reaction
- calculate the value of the equilibrium constant for a reverse reaction from its value for a forward reaction, and if the stoichiometry is changed
- calculate the equilibrium constant for a reaction obtained by combining two other reactions
- calculate equilibrium compositions from starting compositions and the equilibrium constant for a simple gas phase reaction
- calculate the equilibrium composition for a chemical reaction from its equilibrium constant and mass balance information
- use appropriate aproximations for simplifying such calculations
- define the reaction quotient and use it to predict the direction of change in a reaction as it approaches equilibrium, or if it is perturbed from equilibrium.
- use the enthalpy of reaction to predict how the equilibrium constant changes with temperature
- explain that catalysts change the pathway and rate of reaction but not the position of equilibrium
- explain that entropy depends on concentration, but enthalpy can be treated as independent of concentration
- explain the reasons for the conditions used in the Haber Process, and apply the same reasoning to the optimization of other chemical processes, such as smelting
Textbook and eBook References
ChemCAL, iChem and Contributed Resources
Using ICE tables
Description: Tutorial on using ICE tables to solve chemical equilibrium problems
Tags: equilibrium | ICE tables
Contributed by Adam Bridgeman
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