(A) For an ideal mixture,the partial pressure of a component $i$ in the vapour phase is given by $P_i = P_i^o X_i$.Given the molar ratio is $1:1$,the

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The vapour will contain higher percentage of benzene

(A) For an ideal mixture,the partial pressure of a component $i$ in the vapour phase is given by $P_i = P_i^o X_i$.Given the molar ratio is $1:1$,the mole fractions are $X_{benzene} = 0.5$ and $X_{toluene} = 0.5$.The partial pressures are $P_{benzene} = 75 \times 0.5 = 37.5 \, mm \, Hg$ and $P_{toluene} = 22 \times 0.5 = 11 \, mm \, Hg$.The mole fraction in the vapour phase is $Y_i = P_i / P_{total}$.Since $P_{benzene} > P_{toluene}$,it follows that $Y_{benzene} > Y_{toluene}$.Therefore,the vapour will contain a higher percentage of benzene.

Class 12 Chemistry Solutions Ideal and Non-ideal solution

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Which statement about the composition of vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume the temperature is constant at $25\,^{\circ}C$. Vapour pressure data $(25\,^{\circ}C)$:
Benzene: $75\, mm\, Hg$
Toluene: $22\, mm\, Hg$

A
The vapour will contain higher percentage of benzene
B
The vapour will contain higher percentage of toluene
C
The vapour will contain equal amount of benzene and toluene
D
Not enough information is given to make a prediction

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Ideal and Non-ideal solution

Which of the following liquid pairs shows a positive deviation from Raoult's law?

MediumAIEEE 2004

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Which property is shown by an ideal solution?

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The vapour pressures of chloroform $(CHCl_3)$ and dichloromethane $(CH_2Cl_2)$ at $298 \ K$ are $200 \ mmHg$ and $415 \ mmHg$,respectively. An ideal solution is prepared by mixing $59.75 \ g$ of $CHCl_3$ and $21.25 \ g$ of $CH_2Cl_2$. The mole fractions of chloroform and dichloromethane in the vapour phase,respectively,are:

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$1 \, \text{mole}$ of liquid $A$ and $2 \, \text{mole}$ of liquid $B$ form a solution with a vapor pressure of $38 \, \text{torr}$. If the vapor pressures of pure $A$ and pure $B$ are $45 \, \text{torr}$ and $36 \, \text{torr}$ respectively,the solution will be:

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At $373 \ K$,heptane and octane form an ideal solution. The vapor pressures of the two pure liquid components (heptane and octane) are $105 \ kPa$ and $45 \ kPa$,respectively. The vapor pressure of the solution formed by mixing $25 \ g$ of heptane and $35 \ g$ of octane is ........ $kPa$. (Molar masses of heptane and octane are $100 \ g \ mol^{-1}$ and $114 \ g \ mol^{-1}$,respectively.)

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Which statement about the composition of vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume the temperature is constant at $25\,^{\circ}C$. Vapour pressure data $(25\,^{\circ}C)$:Benzene: $75\, mm\, Hg$Toluene: $22\, mm\, Hg$

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Which of the following liquid pairs shows a positive deviation from Raoult's law?

Which property is shown by an ideal solution?

$1 \, \text{mole}$ of liquid $A$ and $2 \, \text{mole}$ of liquid $B$ form a solution with a vapor pressure of $38 \, \text{torr}$. If the vapor pressures of pure $A$ and pure $B$ are $45 \, \text{torr}$ and $36 \, \text{torr}$ respectively,the solution will be:

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Which statement about the composition of vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume the temperature is constant at $25\,^{\circ}C$. Vapour pressure data $(25\,^{\circ}C)$:
Benzene: $75\, mm\, Hg$
Toluene: $22\, mm\, Hg$