Liquids A and B form an ideal solution. If X_ | vedclass

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(B) For an ideal solution,the partial pressure of component $A$ is given by $P_A = X_A P_A^{\circ}$ and the total pressure is $P_{total} = X_A P_A^{\c

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$\frac{Y_A}{X_A} > 1$

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(B) For an ideal solution,the partial pressure of component $A$ is given by $P_A = X_A P_A^{\circ}$ and the total pressure is $P_{total} = X_A P_A^{\circ} + X_B P_B^{\circ}$.According to Dalton's law of partial pressures,$P_A = Y_A P_{total}$.Equating the two expressions for $P_A$: $Y_A P_{total} = X_A P_A^{\circ} \Rightarrow \frac{Y_A}{X_A} = \frac{P_A^{\circ}}{P_{total}}$.Since $P_A^{\circ} > P_B^{\circ}$,the component with the higher vapour pressure will be more concentrated in the vapour phase than in the liquid phase.Therefore,$Y_A > X_A$,which implies $\frac{Y_A}{X_A} > 1$.

Liquids $A$ and $B$ form an ideal solution. If $X_A$ and $Y_A$ are the mole fractions of $A$ in the solution and in vapour phase in equilibrium,respectively,then (Given $P_A^{\circ} > P_B^{\circ}$):

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