Equilibrium as a dynamic model – basic principles
How it works
Chemical equilibrium describes a state in a closed system in which the rate of the forward reaction and the reverse reaction are equal. The concentrations of the substances involved then no longer change, although both reactions continue to take place. It is a dynamic equilibrium. The equilibrium can be influenced by changes in concentration and by changes in temperature. Changes in pressure are especially relevant for equilibria involving gases when the number of gas particles differs between reactants and products. In simplified school form, the law of mass action describes the relationship between the equilibrium constant and the concentrations of reactants and products at equilibrium.
In chemical equilibrium, the forward and reverse reactions proceed in a closed system at the same rate, so that the concentrations of the substances involved remain constant, although the reactions continue to take place.
An example
What does it mean when a chemical reaction in a closed system is at equilibrium?
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50 Exercises
To the learning unit →Own explanation and own practice exercises by AmyMath. Subject reference framework: Chemistry. The topic assignment may vary by federal state.