Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 11: Problem 58

Calculate the solubility of \(\mathrm{O}_{2}\) in water at a partial pressure of \(\mathrm{O}_{2}\) of 120 torr at \(25^{\circ} \mathrm{C}\) . The Henry's law constant for \(\mathrm{O}_{2}\) is $1.3 \times 10^{-3} \mathrm{mol} / \mathrm{L} \cdot\( atm for Henry's law in the form \)C=k P\( where \)C$ is the gas concentration \((\mathrm{mol} / \mathrm{L})\)

Short Answer

Expert verified
The solubility of O₂ in water at a partial pressure of 120 torr and at \(25^{\circ}\)C is approximately \(2.053 \times 10^{-4}\, \text{mol/L}\).

Step by step solution

01

Convert partial pressure from torr to atm

First, we need to convert the given partial pressure of O₂ from torr to atm. Recall the conversion factor: 1 atm = 760 torr. Divide the given partial pressure by 760 to obtain the pressure in atm: \[ P_{O_{2}} = \frac{120 \,\text{torr}}{760\, \text{torr/atm}} \]
02

Find the partial pressure of O₂ in atm

Calculate the partial pressure in atm: \[ P_{O_{2}} = 0.1579 \,\text{atm}\]
03

Use Henry's law to calculate the solubility of O₂

Now we will use the Henry's law formula, which is given as: \[ C = kP \] Where \(C\) is the concentration of the gas in mol/L, \(k\) is the Henry's law constant, and \(P\) is the partial pressure of the gas in atm. We are given \(k = 1.3 \times 10^{-3}\, \text{mol/L} \cdot \text{atm}\) and we found \(P = 0.1579\) atm in Step 2. Substitute these values into the Henry's law formula to find the concentration of O₂: \[ C = (1.3 \times 10^{-3}\, \text{mol/L} \cdot \text{atm}) \times 0.1579 \,\text{atm} \]
04

Calculate the concentration of O₂

Calculate the concentration of O₂ in water: \[ C = 2.053 \times 10^{-4}\, \text{mol/L} \] Thus, the solubility of O₂ in water at a partial pressure of 120 torr and at \(25^{\circ}\)C is approximately \(2.053 \times 10^{-4}\, \text{mol/L}\).

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

At \(25^{\circ} \mathrm{C},\) the vapor in equilibrium with a solution containing carbon disulfide and acetonitrile has a total pressure of 263 torr and is 85.5 mole percent carbon disulfide. What is the mole fraction of carbon disulfide in the solution? At \(25^{\circ} \mathrm{C}\) , the vapor pressure of carbon disulfide is 375 torr. Assume the solution and vapor exhibit ideal behavior.

For each of the following pairs, predict which substance is more soluble in water. a. \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) or \(\mathrm{NH}_{3}\) b. \(\mathrm{CH}_{3} \mathrm{CN}\) or \(\mathrm{CH}_{3} \mathrm{OCH}_{3}\) c. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) or $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}$ d. \(\mathrm{CH}_{3} \mathrm{OH}\) or $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ e. \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CCH}_{2} \mathrm{OH}\) or \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{6} \mathrm{OH}\) f. \(\mathrm{CH}_{3} \mathrm{OCH}_{3}\) or $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$

A \(0.10-m\) NaCl aqueous solution has a higher boiling point than a $0.10-m \mathrm{MgSO}_{4}$ aqueous solution. Explain why.

Table sugar \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) or urea \(\left[\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\right]\) can be used by road crews to melt ice on roads, but solutions of \(\mathrm{CaCl}_{2}\) are generally used instead. Assuming equal costs per pound of substance, why is \(\mathrm{CaCl}_{2}\) used instead of table sugar or urea?

Rubbing alcohol contains 585 g isopropanol $\left(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\right)$ per liter (aqueous solution). Calculate the molarity.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

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