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ChemistryIdeal GasProblems related with container/piston/SPMMedium2 minQB

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Passage / Comprehension

A container is divided into two compartments. One compartment contains 2 moles of N₂ gas at 1 atm and 300 K, while the other compartment contains H₂ gas at the same temperature and pressure. The volume of the H₂ compartment is four times the volume of the N₂ compartment.

[Assuming no reaction under these conditions]

If the container containing $N_{2} & H_{2}$ are further heated to 1000 K , forming $NH_{3}$ with $100%$ yield. Calculate the final total pressure.

Options:

Answer:

Solution:

At 1000 K,

$N_{2} + 3 H_{2} \to 2 NH_{3}$

Initial moles: 2 8 -

Final moles: - 2 4

The total number of moles is $n_{T} = 6$ moles.

The total pressure is $P_{T} = \frac{6 \times 0.0821 \times 1000}{5 \times 49.26} = 2 a t m$ .

Stream:JEESubject:ChemistryTopic:Ideal GasSubtopic:Problems related with container/piston/SPM

⏱ 2mℹ️ Source: QB

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