Dynamic equilibrium in physical and chemical changes, the law of mass action, Kc and Kp and how they are linked, the reaction quotient, finding equilibrium amounts, and Le Chatelier's principle.
3 lessons, about 1 h 15 min3 simulations11 problems3 practice questionsPython in every lesson
Created by StemPy LabMany changes stop short in a closed container: the forward and backward processes keep going at equal rates, so nothing seems to change. This is dynamic equilibrium. It happens in physical changes, such as liquid and vapour or a saturated solution, and in reversible chemical reactions, which reach the same mixture from either side.
For , the law of mass action gives , constant at a given temperature. With partial pressures, . Pure solids and liquids are left out. A large K means products are favoured. Comparing with tells which way a mixture moves.
Le Chatelier's principle: if a change of concentration, pressure or temperature disturbs an equilibrium, the system shifts to undo part of the change. Adding a reactant or removing a product shifts it forward. Raising the pressure favours fewer moles of gas. Only temperature changes K. A catalyst changes neither K nor the mixture, only how fast it is reached.
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