Calculating the Equilibrium Constant
The equilibrium constant (K) quantifies the ratio of product concentrations to reactant concentrations at equilibrium for a reversible reaction.
Key Concepts
- For a reaction: aA + bB ⇌ cC + dD
- Equilibrium constant: K = [C]^c [D]^d / [A]^a [B]^b
- Units of K depend on the reaction stoichiometry, but K is often treated as unitless
- K >> 1: products favored
- K << 1: reactants favored
Steps to Calculate K
- Write the balanced chemical equation
- Determine equilibrium concentrations of all species
- Substitute concentrations into the K expression
- Solve for K
Example
For N₂ + 3 H₂ ⇌ 2 NH₃, if [NH₃] = 0.50 M, [N₂] = 0.25 M, [H₂] = 0.75 M:
K = [NH₃]^2 / ([N₂][H₂]^3)
K = (0.50)^2 / (0.25 × 0.75^3) ≈ 1.78
Importance
- Predicts the extent of a reaction
- Helps in reaction optimization and industrial chemical processes
- Essential for understanding chemical equilibria
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