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Asked Feb 20, 2020
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1-Propanol (P°i = 20.9 Torr at 25 °C) and 2-propanol (P2 = 45.2 Torr at 25 °C) form ideal solutions in all proportions.
Let æ1 and æ2 represent the mole fractions of 1-propanol and 2-propanol in a liquid mixture, respectively, and y, and y2
represent the mole fractions of each in the vapor phase.
For a solution of these liquids with æ1 = 0.560, calculate the composition of the vapor phase at 25 °C.
Y2 =
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1-Propanol (P°i = 20.9 Torr at 25 °C) and 2-propanol (P2 = 45.2 Torr at 25 °C) form ideal solutions in all proportions. Let æ1 and æ2 represent the mole fractions of 1-propanol and 2-propanol in a liquid mixture, respectively, and y, and y2 represent the mole fractions of each in the vapor phase. For a solution of these liquids with æ1 = 0.560, calculate the composition of the vapor phase at 25 °C. Y2 =

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Expert Answer

Step 1

According to Raoult’s law :

Chemistry homework question answer, step 1, image 1

Step 2

Given,

Vapour pressure of 1-propanol (component 1), P1o = 20.9 torr

Vapour pressure of 2-propanol (component 2), P2o = 45.2 torr

Mole fraction of 1-propanol, x1 = 0.560

 

The mole fraction of 2-propanol, x2 can be calculated as:

Chemistry homework question answer, step 2, image 1

Step 3

Partial vapour pressure of 1-propanol and 2-propanol can be calculated as:

Chemistry homework question answer, step 3, image 1

The vapour pressure of the mixture can be calculated as :

Chemistry homework question answer, step 3, image 2

 

...

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