(A) According to Raoult's Law,the total vapour pressure of the solution is given by $P_{total} = X_A P_A^o + X_B P_B^o$.Given $X_B = 0.5$,therefore $X

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(A) According to Raoult's Law,the total vapour pressure of the solution is given by $P_{total} = X_A P_A^o + X_B P_B^o$.Given $X_B = 0.5$,therefore $X_A = 1 - 0.5 = 0.5$.$P_{total} = (0.5 \times 400) + (0.5 \times 600) = 200 + 300 = 500\, mm\, Hg$.Now,the mole fraction of component $A$ in the vapour phase $(Y_A)$ is calculated as $Y_A = \frac{P_A}{P_{total}} = \frac{X_A P_A^o}{P_{total}} = \frac{0.5 \times 400}{500} = 0.4$.Similarly,the mole fraction of component $B$ in the vapour phase $(Y_B)$ is $Y_B = 1 - Y_A = 1 - 0.4 = 0.6$.Thus,the values are $500\, mm\, Hg, 0.4, 0.6$.

Class 12 Chemistry Solutions Lowering of vapour pressure

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The vapour pressures of pure liquids $A$ and $B$ are $400$ and $600\, mm\, Hg$,respectively at $298\, K$. On mixing the two liquids,the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquid $B$ is $0.5$ in the mixture. The vapour pressure of the final solution,the mole fractions of components $A$ and $B$ in vapour phase,respectively are

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A
$500\, mm\, Hg, 0.4, 0.6$
B
$500\, mm\, Hg, 0.5, 0.5$
C
$450\, mm\, Hg, 0.5, 0.5$
D
$450\, mm\, Hg, 0.4, 0.6$

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At $298 \ K$,$0.714$ moles of liquid $A$ is dissolved in $5.555$ moles of liquid $B$. The vapour pressure of the resultant solution is $475 \ torr$. The vapour pressure of pure liquid $A$ at the same temperature is $280.7 \ torr$. What is the vapour pressure of pure liquid $B$ in $torr$?

MediumAP EAMCET 2025

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The vapour pressure of water at $23^{\circ} C$ is $19.8 \ mm$. If $0.1 \ mole$ of glucose is dissolved in $178.2 \ g$ of water, what is the vapour pressure (in $mm$) of the resultant solution?

DifficultAP EAMCET 2005

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The vapour pressure of water at $20\,^{\circ}C$ is $17.5\, mm\, Hg.$ If $18\, g$ of glucose $(C_6H_{12}O_6)$ is added to $178.2\, g$ of water at $20\,^{\circ}C,$ the vapour pressure of the resulting solution will be $.........\, mm$ of $Hg$.

DifficultAIEEE 2008

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Among acetone,ether,and ethanol,which one will have the maximum and which one will have the minimum vapor pressure?

Easy

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Which one of the following represents the graph between $\log p$ (on $Y$-axis) and $\frac{1}{T}$ (on $X$-axis)?
($p=$ vapour pressure of a liquid, $T=$ absolute temperature)

MediumAP EAMCET 2003

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At $298 \ K$,$0.714$ moles of liquid $A$ is dissolved in $5.555$ moles of liquid $B$. The vapour pressure of the resultant solution is $475 \ torr$. The vapour pressure of pure liquid $A$ at the same temperature is $280.7 \ torr$. What is the vapour pressure of pure liquid $B$ in $torr$?

The vapour pressure of water at $23^{\circ} C$ is $19.8 \ mm$. If $0.1 \ mole$ of glucose is dissolved in $178.2 \ g$ of water, what is the vapour pressure (in $mm$) of the resultant solution?

The vapour pressure of water at $20\,^{\circ}C$ is $17.5\, mm\, Hg.$ If $18\, g$ of glucose $(C_6H_{12}O_6)$ is added to $178.2\, g$ of water at $20\,^{\circ}C,$ the vapour pressure of the resulting solution will be $.........\, mm$ of $Hg$.

Among acetone,ether,and ethanol,which one will have the maximum and which one will have the minimum vapor pressure?

Which one of the following represents the graph between $\log p$ (on $Y$-axis) and $\frac{1}{T}$ (on $X$-axis)?($p=$ vapour pressure of a liquid, $T=$ absolute temperature)

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Which one of the following represents the graph between $\log p$ (on $Y$-axis) and $\frac{1}{T}$ (on $X$-axis)?
($p=$ vapour pressure of a liquid, $T=$ absolute temperature)