Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 52

The vapor pressures of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) and 1 -propanol \(\left(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\right)\) at \(35^{\circ} \mathrm{C}\) are \(100 \mathrm{mmHg}\) and \(37.6 \mathrm{mmHg},\) respectively. Assume ideal behavior and calculate the partial pressures of ethanol and 1 -propanol at \(35^{\circ} \mathrm{C}\) over a solution of ethanol in I-propanol, in which the mole fraction of ethanol is 0.300

Short Answer

Expert verified
The partial pressures of ethanol and 1-propanol at \(35^{\circ} C\) over a solution of ethanol in 1-propanol, in which the mole fraction of ethanol is 0.300, are \(30.0 mmHg \) and \(26.32 mmHg\), respectively.

Step by step solution

01

Calculate mole fraction of 1-propanol

We begin by calculating the mole fraction of 1-propanol in the solution. Since the sum of the mole fractions of all the components in a solution equals to 1, the mole fraction of 1-propanol \(X_{C_{3}H_{7}OH}\) can be calculated as \(1 - 0.300 = 0.700\)
02

Calculate partial pressure of ethanol

Next, we calculate the partial pressure of ethanol using Raoult's Law. According to Raoult's Law, the partial pressure of a component in an ideal mixture is the product of the mole fraction of the component and the vapour pressure of the pure component. Here, \(P_{C_{2}H_{5} OH} = X_{C_{2} H_{5} OH} . P^0_{C_{2}H_{5} OH} = 0.300 . 100 mmHg = 30.0 mmHg\)
03

Calculate partial pressure of 1-propanol

Finally, we calculate the partial pressure of 1-propanol using Raoult's Law. For 1-propanol, \(P_{C_{3}H_{7}OH} = X_{C_{3}H_{7}OH} . P^0_{C_{3}H_{7}OH} = 0.700 . 37.6 mmHg = 26.32 mmHg\)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The solubility of \(\mathrm{N}_{2}\) in blood at \(37^{\circ} \mathrm{C}\) and at a partial pressure of \(0.80 \mathrm{~atm}\) is \(5.6 \times 10^{-4} \mathrm{~mol} / \mathrm{L}\). A deepsea diver breathes compressed air with the partial pressure of \(\mathrm{N}_{2}\) equal to \(4.0 \mathrm{~atm} .\) Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of \(\mathrm{N}_{2}\) gas released (in liters) when the diver returns to the surface of the water, where the partial pressure of \(\mathrm{N}_{2}\) is \(0.80 \mathrm{~atm}\)

Explain why it is essential that fluids used in intravenous injections have approximately the same osmotic pressure as blood.

Explain why ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) is not soluble in cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right) .\)

Define boiling-point elevation and freezing-point depression. Write the equations relating boilingpoint elevation and freezing-point depression to the concentration of the solution. Define all the terms, and give their units.

Define the van't Hoff factor. What information does this quantity provide?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free