An amount of 16 moles H₂ and 4 moles of N₂ is confined in a vessel of volume one litre. The vessel is heated to a constant temperature until the equilibrium is established. At equilibrium, the pressur

Question

An amount of 16 moles H₂ and 4 moles of N₂ is confined in a vessel of volume one litre. The vessel is heated to a constant temperature until the equilibrium is established. At equilibrium, the pressure was found to be 9/10ᵗʰ of the initial pressure. The value of K_c for the reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g), is

Prashant Kotian · Accepted Answer

Correct answer: B. Initial moles = 20. Equilibrium moles = 20 × (9/10) = 18. Let x moles of N₂ react. Eq moles: N₂ = 4-x, H₂ = 16-3x, NH₃ = 2x. Total moles = 20 - 2x = 18, so x = 1. Eq concentrations: [N₂] = 3 M, [H₂] = 13 M, [NH₃] = 2 M. K_c = (2)² / (3 × 13³) = 4 / (3 × 2197) = 4 / 6591 ≈ 6.068 × 10⁻⁴. Therefore, correct answer is B.

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