For dissociation of ammonia gas as: 2NH 3 (g) ⇌ N 2 (g) + 3H 2 (g). The reaction is performed at constant temperature and volume. If D is the vapour density of the equilibrium mixture, P o is the init

Question

For dissociation of ammonia gas as: 2NH 3 (g) ⇌ N 2 (g) + 3H 2 (g). The reaction is performed at constant temperature and volume. If D is the vapour density of the equilibrium mixture, P o is the initial pressure of NH 3 (g) and M is the molecular mass of NH 3 , then the correct information(s) at equilibrium is/are

TestHub · Accepted Answer

Take 1 mol of NH 3 initially: NH 3 = 1 - α, N 2 = α/2, H 2 = 3α/2 Total moles = 1 + α Mass is conserved, so M/M avg = 1 + α with M avg = 2D α = (M - 2D)/(2D), so (b) is incorrect since it gives twice this value At constant V and T, P = P o (1 + α) = P o M/(2D), so (a) is correct P NH3 = P o (1 - α) = P o (2D - M + 2D)/(2D) = (4D - M)P o /(2D), so (c) is correct P H2 = 3P o α/2 = 3(M - 2D)P o /(4D), so (d) is correct The correct options are (a), (c) and (d).

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