In the reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat. One mole of N₂ reacts with three moles of H₂. If at equilibrium 'x' moles of N₂ combined, then the value of 'x' in terms of K_p and the total pressure

Question

In the reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat. One mole of N₂ reacts with three moles of H₂. If at equilibrium 'x' moles of N₂ combined, then the value of 'x' in terms of K_p and the total pressure of gases at equilibrium, P, is

Prashant Kotian · Accepted Answer

Correct answer: A. Eq moles: N₂ = 1-x, H₂ = 3(1-x), NH₃ = 2x. Total moles = 4 - 2x = 2(2-x). Partial pressures: P_NH₃ = xP/(2-x), P_N₂ = (1-x)P/(2(2-x)), P_H₂ = 3(1-x)P/(2(2-x)). Assuming x is very small (1-x ≈ 1, 2-x ≈ 2), K_p = (xP/2)² / [ (P/4) × (3P/4)³ ] = (x²P²/4) / (27P⁴/256) = 64x² / 27P². Solving for x gives x = 3P√(3K_p) / 8. Therefore, correct answer is A.

💡 Solution & Explanation

Practice 22,000+ questions like this