Vapour pressure of pure acetone and chloroform at $328 \, K$ are $741.8 \, mm \, Hg$ and $632.8 \, mm \, Hg$ respectively. Assuming that they form an ideal solution over the entire range of composition,plot $p_{total}$,$p_{chloroform}$,and $p_{acetone}$ as a function of $x_{acetone}$. The experimental data observed for different compositions of the mixture is:
$100 \times x_{acetone}$ $0, 11.8, 23.4, 36.0, 50.8, 85.2, 64.5, 72.1$ $p_{acetone} / mm \, Hg$ $0, 54.9, 110.1, 202.4, 322.7, 405.9, 454.1, 521.1$ $p_{chloroform} / mm \, Hg$ $632.8, 548.1, 469.4, 359.7, 257.7, 193.6, 161.2, 120.7$
| $100 \times x_{acetone}$ | $0, 11.8, 23.4, 36.0, 50.8, 85.2, 64.5, 72.1$ |
| $p_{acetone} / mm \, Hg$ | $0, 54.9, 110.1, 202.4, 322.7, 405.9, 454.1, 521.1$ |
| $p_{chloroform} / mm \, Hg$ | $632.8, 548.1, 469.4, 359.7, 257.7, 193.6, 161.2, 120.7$ |
(N/A) To determine the deviation from ideal behaviour,we calculate the total pressure $p_{total} = p_{acetone} + p_{chloroform}$ for each composition:
By plotting the experimental $p_{total}$ against $x_{acetone}$,we observe that the curve lies below the straight line expected for an ideal solution. This indicates that the mixture of acetone and chloroform exhibits negative deviation from Raoult's law.
| $100 \times x_{acetone}$ | $0, 11.8, 23.4, 36.0, 50.8, 85.2, 64.5, 72.1$ |
| $p_{total} / mm \, Hg$ | $632.8, 603.0, 579.5, 562.1, 580.4, 599.5, 615.3, 641.8$ |
By plotting the experimental $p_{total}$ against $x_{acetone}$,we observe that the curve lies below the straight line expected for an ideal solution. This indicates that the mixture of acetone and chloroform exhibits negative deviation from Raoult's law.
Explore More
Similar Questions
In a mixture of components $A$ and $B$,the components show negative deviation when:
MediumAIEEE 2002
View SolutionSolution $A$ contains acetone dissolved in chloroform and solution $B$ contains acetone dissolved in carbon disulphide. The type of deviations from Raoult's law shown by solutions $A$ and $B$,respectively,are:
Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.
An ideal solution is that which
Medium
View SolutionWhich one is an example of an ideal solution from the following?
Vedclass 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