Chemistry - Ideal Gas Question with Solution | TestHub
ChemistryIdeal GasProblems related with container/piston/SPMEasy2 minQB
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Passage / Comprehension
The apparatus shown consists of three temperature jacketed 1.642 l bulbs connected by stopcocks. Bulb A contains a mixture of H₂O(g), CO₂(g) and N₂(g) at 27°C and a total pressure of 684 mm Hg. Bulb B is empty and held at -73°C. Bulb C is also empty and held at -193°C. The stopcocks are closed and the volume of the connecting lines is zero. CO₂ sublimes at -78°C and N₂ boils at -196°C. Neglect the volume of any solid, if formed.
How many moles of H₂O are in the system?
Options:
Answer:
C
Solution:
Total moles = ((684/760) × 1.642)/(0.0821 × 300) = 0.9 × 1.642/24.63 = 0.06 mol. Gas (CO₂ + N₂) = 0.04 mol. n(H₂O) = 0.06 - 0.04 = 0.02 mol. Hence (c).
Stream:JEESubject:ChemistryTopic:Ideal GasSubtopic:Problems related with container/piston/SPM
⏱ 2mℹ️ Source: QB
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