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tangare [24]
3 years ago
8

Two alcohols, isopropyl alcohol and propyl alcohol, have the same molecular formula, C3H8O. A solution of the two that is two-th

irds by mass isopropyl alcohol has a vapor pressure of 0.110 atm at 313 K. A solution that is one-third by mass isopropyl alcohol has a vapor pressure of 0.089 atm at 313 K. 1. Calculate the vapor pressure of each pure alcohol at this temperature.2. Explain the difference given that the formula of propyl alcohol is CH3CH2CH2OH and that of isopropyl alcohol is (CH3)2CHOH.
Chemistry
1 answer:
iris [78.8K]3 years ago
5 0

Answer:

1.

Since both components of these solutions have the same molar mass, mole fractions would be the same as mass fractions.

0.110 atm = (2/3)(Pi) + (1/3)(Pn) [1]

0.089 atm = (1/3)(Pi) + (2/3)(Pn) [2]

2*[1] - [2]:

(2)(0.110) - 0.089 atm = Pi

Pi = 0.131 atm

2*[2] - [1]:

(2)(0.089) - 0.110 atm = Pn

Pn = 0.068 atm

2.

The hydroxyl (-OH) group on the end of a longer 1-propanol molecule makes it more polar than IPA. It follows that the intermolecular forces between 1-propanol are stronger than those of IPA and thus the vapor pressure of 1-propanol should be lower than IPA.

Explanation:

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Answer:

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Explanation:

Let us first consider the molar Masses of each gas

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Looking at the gases listed, C2H6 have the highest average kinetic energy at this temperature since it has the lowest molecular mass. This reasoning is directly derived from Graham's law of diffusion in gases.

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