At $300 \ K$,the vapour pressures of $A$ and $B$ liquids are $500 \ mm \ Hg$ and $400 \ mm \ Hg$ respectively. Equal moles of $A$ and $B$ are mixed to form an ideal solution. The mole fraction of $A$ and $B$ in the vapor state is respectively:
- A$0.5, 0.5$
- B$0.666, 0.333$
- C$0.444, 0.555$
- D$0.555, 0.444$
Explore More
Similar Questions
Which from the following liquid mixtures behaves nearly as an ideal solution?
$A$ mixture of toluene and benzene forms a nearly ideal solution. Assume $p_{B}^{\circ}$ and $p_{T}^{\circ}$ to be the vapour pressures of pure benzene and toluene,respectively. The slope of the line obtained by plotting the total vapour pressure versus the mole fraction of benzene is $....$
MediumKVPY 2020
View SolutionWhich of the following mixtures is a non-ideal solution?
In a mixture of $A$ and $B$ components,the solution shows positive deviation from Raoult's law when:
Medium
View SolutionWhich one of the following is incorrect for an ideal solution?
MediumNEET 2016
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo