The vapour pressure of chloroform $({C H C l}_{3})$ and dichloromethane $({C H}_{2} {C l}_{2})$ at 298 K is 200 mm Hg and 415 mm Hg, respectively. If a solution is prepared by mixing 25.5 g of ${C H C l}_{3}$ and 40 g of ${C H}_{2} {C l}_{2}$ at 298 K, calculate the mole fractions of chloroform in vapour phase.

0.18

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0.82

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0.34

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0.48

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Solution

The correct option is A $0.18$
$\begin{matrix} Calculate the VP of solution mass of {C H C l}_{3} = 25.5 g mass of {C H}_{2} {C l}_{2} = 40 g \end{matrix}$

$mole of {C H C l}_{3} = \frac{25.5 g}{119 .5 g {m o l}^{- 1}}$

$= 0.213 m o l e$
$mole o f {C H}_{2} {C l}_{2} = \frac{40}{85} = 0.470 m o l$

$\begin{matrix} mole Fraction of {C H}_{2} {C l}_{2} = 1 P T = 347 . 9 m m \end{matrix}$
$mole fraction of CHCl3(yCHCl3)=PCHCl3PTotal in vapour phase$

$\begin{matrix} = \frac{62.4 m m}{347.9 m m} = 0.18 \end{matrix}$

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Q. The vapour pressure of chloroforms and de-chloroforms at 298 k are 200 mm Hg and 415 mm Hg? calculate the vapour pressure of solution by mixing 25.5 gram of

C H C l_{3}

40 gram of

C H_{2} C l_{2}

. calculate the mole fraction of each component on vapour phase.

(a) Vapour pressure of chloroform $(C H C l_{3})$ and dichloromethane $(C H_{2} C l_{2})$ at 298 K are 200 mm Hg and 415 mm Hg respectively. Calculate the vapour pressure of the solution prepared by mixing 25.5 g of CHCl3 and 40 g of $C H_{2} C l_{2} a t 298 K$