At 27^{circ} C,two liquids A and B form an id | vedclass

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(A) According to Raoult's law for an ideal solution,the total vapour pressure $P_{total}$ is given by the sum of the partial pressures of the componen

Vedclass · Accepted Answer

$349.5$

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(A) According to Raoult's law for an ideal solution,the total vapour pressure $P_{total}$ is given by the sum of the partial pressures of the components: $P_{total} = P_A + P_B$. Given: Mole fraction of $A$ $(x_A)$ = $0.67$ Mole fraction of $B$ $(x_B)$ = $0.33$ Vapour pressure of pure $A$ $(P^{\circ}_A)$ = $300 \ mm$ Vapour pressure of pure $B$ $(P^{\circ}_B)$ = $450 \ mm$ Using the formula $P_{total} = x_A P^{\circ}_A + x_B P^{\circ}_B$: $P_{total} = (0.67 	imes 300) + (0.33 	imes 450)$ $P_{total} = 201 + 148.5 = 349.5 \ mm$.

At $27^{\circ} C$,two liquids $A$ and $B$ form an ideal solution with mole fractions $0.67$ and $0.33$ respectively. If the vapour pressure of pure $A$ and $B$ at $27^{\circ} C$ are $300 \ mm$ and $450 \ mm$ respectively,the total vapour pressure of the solution in $mm$ is:

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