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The vapor pressure of methanol, $\mathrm{CH}_{3} \mathrm{OH},$ is 94 torr at $20^{\circ} \mathrm{C}$ . The vapor pressure of ethanol, is 44 torr at the same temperature(a) Calculate the mole fraction of methanol and of ethanol in a solution of 50.0 g of methanol and 50.0 g of ethanol.(b) Ethanol and methanol form a solution that behaves like an ideal solution. Calculate the vapor pressure of methanol and of ethanol above the solution at $20^{\circ} \mathrm{C}$.(c) Calculate the mole fraction of methanol and of ethanol in the vapor above the solution.

a. 0.59 , 0.41b. 55.46 torr , 18.04 torrc. 0.75 , 0.25

03:14

Aadit S.

Chemistry 102

Chapter 11

Solutions and Colloids

Solutions

University of Central Florida

Rice University

University of Maryland - University College

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this question is a result law question referring to the solution as an ideal solution part A simply wants you to calculate the mole fraction of methanol and ethanol from a solution that is 50 g methanol and 50 g ethanol. To do that. The mole fraction of methanol will be the molds methanol which is the mass. Methanol multiplied. I'm sorry, divided by the molar mass of methanol. They're in the numerator. Then we have moles methanol. We divide that by the total moles of the solution, which will be the molds methanol. Again, it's mass divided by its molar mass plus the moles of ethanol, which would be its mass. 50 g divided by its molar mass, 46.7 g. This gives us a mole fraction of .590 methanol because ethanol is the only other substance in the solution. Then the fraction that is the mole fraction that is ethanol is what is left out of one. So the mole fraction ethanol is .410 part B. Then asks, um do you to calculate the vapor pressure of the methanol and ethanol above the solution? The vapor pressure of each of these will be there mull fraction multiplied by their vapor pressure when they are pure. So we'll take the mole fraction of ethanol multiplied by the vapor pressure, pure ethanol, and we'll get the vapor pressure of ethanol coming from the solution. 18 tour. We'll do the same thing with methanol. It's Mole fraction multiplied by its vapor pressure when pure and we get 55 4 tour. Now the mole fraction in the vapor phase is simply a ratio of the partial pressures. The mole fraction of methanol and the vapor phase will be its partial pressure divided by the total pressure, Which gives us 754. And then ethanol will simply be what is left out of 1, 2, 4, 6.

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