Chem. Unit 4, Chapter 2 - Equilibria

A summary of the equilibria chapter of unit 4 chemistry.

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  • Created by: Ajay
  • Created on: 07-01-13 20:09
Preview of Chem. Unit 4, Chapter 2 - Equilibria

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Ajay Rai
Some reactions are reversible and when they appear to have stopped, they are actually at
dynamic equilibrium.
Dynamic equilibrium ­ when the concentrations of reactants and products do not change as the
rate of the forward reaction is equal to the rate of the reverse.
If reactants and products are in the same phase, the reaction is homogenous. If reactants and
products are in different phases, the reaction is heterogeneous.
Equilibrium constant Kc ­ the equilibrium constant, Kc, is the ratio of the concentrations of
products and reactants, where c stands for the molar concentration.
The general equation for any homogenous reaction at equilibrium is aA + bB cC + dD, where a,
b, c and d are the numbers of moles of substances A, B, C and D. Kc in this instance is therefore
expressed as Kc =
The equilibrium constant value for a reaction is constant at a fixed temperature.
Factors affecting equilibrium ­ Le Chatelier's principle states that the position of the
equilibrium of a system changes to minimise the effect of any imposed change in conditions.
When different proportions of reactants in a reversible reaction are mixed at fixed temperatures,
the concentrations of the reactants and products will adjust until the value of the equilibrium
constant is achieved.
Catalysts don't affect the position of equilibrium but they do ensure that equilibrium is reached


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