Introduction to Equilibrium
Chemical equilibrium occurs when a reversible reaction reaches a state where the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant over time.
Key Concepts
- Dynamic Equilibrium: Reactions continue, but no net change in concentrations
- Equilibrium Constant (K): Expresses the ratio of product to reactant concentrations at equilibrium
- For aA + bB ⇌ cC + dD: K = [C]^c [D]^d / [A]^a [B]^b
- Reaction Quotient (Q): Used to predict the direction a reaction will shift
- Q < K → reaction shifts forward
- Q > K → reaction shifts reverse
- Q = K → reaction is at equilibrium
Importance
- Predicts composition of chemical mixtures at equilibrium
- Helps in industrial processes like the Haber process
- Explains effects of concentration, pressure, and temperature on reactions (Le Chatelier’s Principle)
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