(B) According to Raoult's law,the total pressure $P_{total}$ is given by $P_{total} = P_{toluene}^0 \chi_{toluene} + P_{benzene}^0 \chi_{benzene}$.Sin

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(B) According to Raoult's law,the total pressure $P_{total}$ is given by $P_{total} = P_{toluene}^0 \chi_{toluene} + P_{benzene}^0 \chi_{benzene}$.Since the mixture boils at $100^{\circ} C$ at $1 \ atm$ pressure,$P_{total} = 1.013 \ bar$.Let $\chi_{toluene} = x$,then $\chi_{benzene} = 1 - x$.Substituting the values: $1.013 = 0.742x + 1.800(1 - x)$.$1.013 = 0.742x + 1.800 - 1.800x$.$1.013 - 1.800 = (0.742 - 1.800)x$.$-0.787 = -1.058x$.$x = \frac{0.787}{1.058} \approx 0.744$.

Class 12 Chemistry Solutions Ideal and Non-ideal solution

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$A$ mixture of toluene and benzene boils at $100^{\circ} C$. Assuming ideal behaviour,the mole fraction of toluene in the mixture is closest to (Vapour pressures of pure toluene and pure benzene at $100^{\circ} C$ are $0.742 \ bar$ and $1.800 \ bar$,respectively. $1 \ atm = 1.013 \ bar$)

KVPY 2017 All KVPY

A
$0.824$
B
$0.744$
C
$0.544$
D
$0.624$

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Ideal and Non-ideal solution

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If liquids $A$ and $B$ form an ideal solution,then:

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In a mixture of $A$ and $B$ components,the solution shows positive deviation from Raoult's law when:

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Liquids $A$ and $B$ form an ideal solution. The vapour pressure of pure $A$ and $B$ are $50 \ mm \ Hg$ and $32 \ mm \ Hg$ respectively at $300 \ K$. One mole of liquid $A$ is mixed with $1$ mole of liquid $B$. What is the approximate mole fraction of $A$ in the vapour phase?

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Solution $A$ 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:

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Which one of the following non-ideal solutions shows negative deviation?

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$A$ mixture of toluene and benzene boils at $100^{\circ} C$. Assuming ideal behaviour,the mole fraction of toluene in the mixture is closest to (Vapour pressures of pure toluene and pure benzene at $100^{\circ} C$ are $0.742 \ bar$ and $1.800 \ bar$,respectively. $1 \ atm = 1.013 \ bar$)

Similar Questions

If liquids $A$ and $B$ form an ideal solution,then:

In a mixture of $A$ and $B$ components,the solution shows positive deviation from Raoult's law when:

Liquids $A$ and $B$ form an ideal solution. The vapour pressure of pure $A$ and $B$ are $50 \ mm \ Hg$ and $32 \ mm \ Hg$ respectively at $300 \ K$. One mole of liquid $A$ is mixed with $1$ mole of liquid $B$. What is the approximate mole fraction of $A$ in the vapour phase?

Solution $A$ 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 one of the following non-ideal solutions shows negative deviation?

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