Dynamic equilibrium, Le Chatelier's principle, the equilibrium constant Kc, and industrial compromise conditions.
A reversible reaction can reach dynamic equilibrium in a closed system: forward and backward rates are equal, and concentrations stay constant (though both reactions continue).
Le Chatelier's principle
If a change is made to a system at equilibrium, the position shifts to oppose the change:
Concentration: adding a reactant shifts right (towards products).
Pressure: increasing pressure shifts to the side with fewer gas moles.
Temperature: increasing temperature shifts in the endothermic direction.
Catalyst: no shift — speeds both directions equally (reaches equilibrium faster).
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