important of equilibrium constant

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Importance of Equilibrium Constant

Equilibrium constant helps predict key features of a chemical reaction:

Determines equilibrium concentration.

Predicts the direction of a chemical reaction.

Predicts the extent of a reaction.

Predicts the effect of changes in conditions.

Industrial applications: Chemists use equilibrium principles to optimize conditions like concentration, temperature, and pressure for efficient production.

Examples of Industrial Applications

1. Haber Process (Ammonia Production)

Reaction:

N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)

- Temperature: 400°C

- Pressure: 200 atm

- Catalyst: Iron

Key Concept: High pressure favors ammonia formation.

2. Contact Process (Sulfuric Acid Production)

Sulfur dioxide purification & oxidation:

2SO_2(g) + O_2(g) 2SO_3(g)

- Temperature: 450°C

- Pressure: 200 atm

- Catalyst: Pt or V₂O₅

Key Concept: Maximizing SO₂ to SO₃ conversion ensures higher sulfuric acid yield.