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.
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