A mixture of N₂ and H₂ in 1:3 mole ratio is used to prepare ammonia by the reaction:
N₂(g) + 3H₂(g) $\to$ 2NH₃(g)
The total pressure of gases in the container is 4.0 atm at 27°C, before the reaction. The final total pressure of gases (in atm) at 127°C after reaction assuming 50% yield of ammonia is

Question

A mixture of N₂ and H₂ in 1:3 mole ratio is used to prepare ammonia by the reaction:

N₂(g) + 3H₂(g) $\to$ 2NH₃(g)

The total pressure of gases in the container is 4.0 atm at 27°C, before the reaction. The final total pressure of gases (in atm) at 127°C after reaction assuming 50% yield of ammonia is

TestHub · Accepted Answer

Before reaction (300 K): P(N₂) = 1.0 atm, P(H₂) = 3.0 atm (stoichiometric ratio).

50% yield: H₂ consumed = 1.5, N₂ consumed = 0.5, NH₃ formed = 1.0 atm-equivalent.

Remaining at 300 K: N₂ = 0.5, H₂ = 1.5, NH₃ = 1.0; total = 3.0 atm.

Scale to 400 K: P_final = 3.0 × 400/300 = 4.0 atm.

Chemistry - Ideal Gas Question with Solution | TestHub

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