At a given temperature the vapor pressure of pure liquid diethyl ether and isopropyl alcohol are 730 torr and 310 torr, respectively. a solution prepared by mixing isopropyl alcohol and diethyl ether obeys raoult's law. at this temperature, what is the vapor pressure of diethyl ether over a solution in which its mole fraction is 0.270?

197.1 torr.

Explanation:

Raoult's law states that the partial vapor pressure of each component of an ideal mixture of liquids is equal to the vapor pressure of the pure component multiplied by its mole fraction in the mixture.Pi = Xi.Pi°, where, Pi is the partial vapor pressure of the component i, Xi is the mole fraction of the component i, and Pi° is the vapor pressure of the pure component i.For diethyl ether; Xi = 0.270, and Pi° = 730.0 torr.So, the vapor pressure of diethyl ether over the solution (Pi diethyl ether) = (0.270 x 730.0) = 197.1 torr.

We first assume that this gas is an ideal gas where it follows the ideal gas equation. the said equation is expressed as: pv = nrt. from this equation, we can predict the changes in the pressure, volume and temperature. if the volume and the temperature of this gas is doubled, then the pressure still stays the same.

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