An ideal solution if obtained by mixing CH3 CHBr2 and CH2Br - CH2Br in the ratio 2-1 PoCH3CHBr2 - 173- PoCH2BrCH2Br - 127- Thus total vapour pressure is-

The correct option is A 158 P = Po_1x_1 + Po_2x_2 x_1 = 22 +1 = 23 x_2 = 13 Total pressure = P Partial pressure of CH_3CHBr_2 = P ...

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Byju's Answer

Standard XII

Chemistry

Raoult's Law

An ideal solu...

Question

An ideal solution if obtained by mixing $C H_{3} C H B r_{2}$ and $C H_{2} B r - C H_{2} B r$ in the ratio $2 : 1$
$P_{C H_{3} C H B r_{2}}^{o} = 173, P_{C H_{2} B r C H_{2} B r}^{o} = 127$ . Thus total vapour pressure is:

158

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Solution

The correct option is A $158$
$P = P o_{1} x_{1} + P o_{2} x_{2}$
$x_{1} = \frac{2}{2 + 1} = \frac{2}{3}$
$x_{2} = \frac{1}{3}$
Total pressure $= P$
Partial pressure of $C H_{3} C H B r_{2} = P o_{1}$
Partial pressure of $C H_{3} B r C H_{2} B r = P o_{2}$
Mole fraction $C H_{3} C H B r_{2} = x_{1}$
Mole fraction $C H_{3} C H B r C H_{2} B r = x_{2}$
$P = 173 \times \frac{2}{3} + 127 \times \frac{1}{3}$
$P = 158$ .

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An ideal solution if obtained by mixing CH3CHBr2 and CH2Br−CH2Br in the ratio 2:1PoCH3CHBr2=173,PoCH2BrCH2Br=127. Thus total vapour pressure is:

The correct option is A 158P=Po1x1+Po2x2x1=22+1=23x2=13Total pressure =PPartial pressure of CH3CHBr2=Po1Partial pressure of CH3BrCH2Br=Po2Mole fraction CH3CHBr2=x1Mole fraction CH3CHBrCH2Br=x2P=173×23+127×13P=158.

An ideal solution if obtained by mixing $C H_{3} C H B r_{2}$ and $C H_{2} B r - C H_{2} B r$ in the ratio $2 : 1$
$P_{C H_{3} C H B r_{2}}^{o} = 173, P_{C H_{2} B r C H_{2} B r}^{o} = 127$ . Thus total vapour pressure is: