Reaction Quotient and Le Châtelier’s Principle
The reaction quotient (Q) helps predict how a system at a given moment will respond, while Le Châtelier’s Principle describes how a system at equilibrium reacts to changes.
Key Concepts
- Reaction Quotient (Q): Q = [products]^coeff / [reactants]^coeff for any point in the reaction
- Comparing Q and K:
- Q < K → reaction shifts forward toward products
- Q > K → reaction shifts reverse toward reactants
- Q = K → system is at equilibrium
- Le Châtelier’s Principle: A system at equilibrium will shift to counteract a disturbance
- Change in concentration, pressure, or temperature will affect Q and the reaction direction
Example
For N₂ + 3 H₂ ⇌ 2 NH₃, ΔH < 0:
- Adding H₂ → Q < K → reaction shifts toward products
- Increasing temperature → system shifts toward reactants
Importance
- Predicts reaction shifts under non-equilibrium conditions
- Integrates quantitative (Q vs. K) and qualitative (Le Châtelier) approaches
- Essential for industrial and laboratory optimization
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