The following concentrations were observed at 500 K for the formation of NH₃ from N₂ and H₂. At equilibrium: [N₂] = 2 × 10⁻² M, [H₂] = 3 × 10⁻² M, and [NH₃] = 1.5 × 10⁻² M. Equilibrium constant for the reaction is ________.

Numerical Answer Type:
Enter a numerical value Answer: 417 to 417 +4 marks

Solution & Explanation

Related Formula
N₂(g) + 3H₂(g) leftharpoons 2NH₃(g) Kc = [NH₃]²[N₂][H₂]³
Core Logic

Substituting the given equilibrium concentrations into the equilibrium constant expression:

Kc = (1.5 × 10⁻²)²(2 × 10⁻²) × (3 × 10⁻²)³

Evaluating the values step-by-step:

Kc = 2.25 × 10⁻⁴(2 × 10⁻²) × (27 × 10⁻⁶)
Step 1: Final Arithmetic Integration
Kc = 2.25 × 10⁻⁴54 × 10⁻⁸ = (2.25)/(54) × 10⁴ = 0.041666 × 10⁴ ≈ 416.67

Rounding to the nearest integer yields 417.

Pattern Recognition

Pay close attention to the cubic exponent in the denominator derived from the hydrogen stoichiometric coefficient (3). Small calculation errors here can significantly alter the result.

Chapter Mix

Class 11 Chemistry: Chemical Equilibrium

More Chemical Equilibrium Previous-Year Questions — Page 8

Q62 jee_main_2024_31_jan_morning Equilibrium Constant
For the given reaction, choose the correct expression of KC from the following :- Fe(aq)³⁺ + SCN(aq)⁻ leftharpoons (FeSCN)(aq)²⁺
  • A. KC = [FeSCN²⁺][Fe³⁺][SCN⁻]
  • B. KC = [Fe³⁺][SCN⁻][FeSCN²⁺]
  • C. KC = [FeSCN²⁺][Fe³⁺]²[SCN⁻]²
  • D. KC = [FeSCN²⁺]²[Fe³⁺][SCN⁻]

Solution

Related Formula
KC = [Products][Reactants]
Core Logic
KC = Products ion conc.Reactants ion conc. KC = [FeSCN²⁺][Fe³⁺][SCN⁻]
Chapter Mix

Class 11 Chemistry: Equilibrium

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