A liquid mixture contains 10 moles of A (P_A | vedclass

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(D) The mole fraction of $A$ $(x_A)$ is $10 / (10 + 10) = 0.5$ and $x_B = 0.5$. According to Raoult's law,the expected vapour pressure is $P_{ideal} =

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None of these

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(D) The mole fraction of $A$ $(x_A)$ is $10 / (10 + 10) = 0.5$ and $x_B = 0.5$. According to Raoult's law,the expected vapour pressure is $P_{ideal} = P_A^0 x_A + P_B^0 x_B = (200 	imes 0.5) + (100 	imes 0.5) = 100 + 50 = 150 \ mm \ Hg$. Since the observed vapour pressure $(160 \ mm \ Hg)$ is greater than the ideal vapour pressure $(150 \ mm \ Hg)$,the solution shows a positive deviation from Raoult's law. For solutions showing positive deviation: $\Delta H_{mix} > 0$,$\Delta V_{mix} > 0$,and $\Delta G_{mix} Since $\Delta H_{mix} > 0$ (endothermic process),the heat is absorbed from the surroundings,so $\Delta S_{surrounding} = -\Delta H_{mix} / T None of the given options $(A, B, C)$ are correct.

$A$ liquid mixture contains $10 \ moles$ of $A$ $(P_A^0 = 200 \ mm \ Hg)$ and $10 \ moles$ of $B$ $(P_B^0 = 100 \ mm \ Hg)$. The vapour pressure over the liquid mixture is $160 \ mm \ Hg$. Which statement is correct?

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