Chemistry - Ideal Gas Question with Solution | TestHub
ChemistryIdeal GasVapour PressureMedium2 minQB
ChemistryMediumnumerical
A container with a volume of 20.0L holds N2(g) and H2O(l) at 300 K. The pressure is found to be 1.0 atm. The water is then split into hydrogen and oxygen by electrolysis. After the reaction is complete, the pressure is 1.86 atm. What mass (in g) of water was present initially in the container? The aqueous tension of water at 300 K is 0.04 atm. (R = 0.08 L-atm/K-mol)
Answer:
9.00
Solution:
Initially: P(N2) = 1.0 - 0.04 = 0.96 atm.
After complete electrolysis all liquid water is gone (no aqueous tension remains); the gases are N2 (0.96 atm-equivalent), H2 = w mol and O2 = w/2 mol, where w = moles of water.
Pfinal = 0.96 + (1.5w)(RT/V) = 1.86 ⇒ 1.5w × (0.08 × 300/20.0) = 0.90 ⇒ 1.5w × 1.2 = 0.90.
1.5w = 0.75 ⇒ w = 0.50 mol ⇒ mass = 0.50 × 18 = 9 g.
Stream:JEESubject:ChemistryTopic:Ideal GasSubtopic:Vapour Pressure
⏱ 2mℹ️ Source: QB
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