Consider a solution containing liquids A and B where the mole fraction of B is 0.60.Assuming ideality,calculate the mole fraction of A in the vapor at equilibrium with this solution at 25°C.(The vapor pressures of pure liquid A and B at 25°C are 117.7 torr and 400.0 torr,respectively. ) A)0.16 B)196 C)0.31 D)3.40 $\times$ 10^-³ E)4.90 $\times$ 10^-³

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Quizplus · Accepted Answer

Raoult's law states that the partial pressure of a component in a vapor is equal to the product of its mole fraction in the liquid and the vapor pressure of the pure component. Therefore, the mole fraction of A in the vapor is:XA = PA / Ptotal = (1 - XB) * PA / (PA + PB) = (1 - 0.60) * 117.7 torr / (117.7 torr + 400.0 torr) = 0.16

Consider a Solution Containing Liquids a and B Where the Mole