Chemistry - Liquid Solution Question with Solution | TestHub

ChemistryLiquid SolutionRaoult's LawMedium2 minPYQ_2010

ChemistryMediumsingle choice

If $1 0^{- 4} dm^{3}$ of water is introduced into a $1.0 dm^{3}$ flask to $300 K$ , how many moles of water are in the vapour phase when equilibrium is established? (Given : Vapour pressure of $H_{2} O$ at $300 K$ is $3170 Pa; R = 8.314 J K^{- 1} mol^{- 1}$ )

Options:

Answer:

Solution:

$n = \frac{PV}{RT} =$ $= 128 \times 1 0^{- 5} moles$ $= \frac{3170 \times 1 0 ^{- 5} atm \times 1 L}{0.0821 L atm k ^{- 1} mol ^{- 1} \times 300K} \approx 1.27 \times 1 0^{- 3} mol$

Stream:JEESubject:ChemistryTopic:Liquid SolutionSubtopic:Raoult's Law

⏱ 2mℹ️ Source: PYQ_2010

Doubts & Discussion

Loading discussions...