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Find the vapour pressure of solution whe...

Find the vapour pressure of solution where 0.5 g pf a nonk volatile solute (Mol wt. =65g) is dissolve in 100mL `"CC"l_(4)`.
Given
Density of `"CC"l_(4)=1.58g//cm^(3)`
Vapour pressure of `"CC"l_(4)` at `25^(@)C` is 143 mm Hg.

Text Solution

Verified by Experts

The correct Answer is:
`142`
Mass of `"CC"l_(4)(W)="Volume"xx"density"`
`=100xx1.58=158g`
Mass of solute (w) =0.5g
`P_(0)=143mmHg,P_(s)=?`
As we know `(P_(0)-P_(s))/(P_(0))=(wxxM)/(mxxW)`
`(143-P_(s))/143=(0.5xx154)/(65xx158)`
`143-P_(S)=(0.5xx154xx143)/(65xx158)`
`143-P_(s)=1.072`
`P_(s)=143-1.072=141.927 mmHg`
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Knowledge Check

  • Vapour pressure of "CCl"_(4) at 25^(@)C is 143 mm Hg . 0.5 g of a non-volatile solute ( molar mass = 65 mol^(-1) ) is dissolved in 100 mL of "CCl"_(4) (density = 1.538g mL^(-1) ) Vapour pressure of solution is :

    A
    `141.9` mm Hg
    B
    `94.4` mmHg
    C
    `99.3` mm Hg
    D
    `144.1` mm Hg

  • The vapour pressure of C Cl_4 at 25^@C is 143 mm Hg, if 0.5 g of a non-volatile solute (mol. weight = 65) is dissolved in 100 g of C CI_4 , the vapour pressure of the solution will be

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    94.39 mm Hg
    B
    199.34 mm Hg
    C
    141.31 mm Hg
    D
    143.99 mm Hg

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    B
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    D
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