   # The partial pressure of O 2 in your lungs varies from 25 mm Hg to 40 mm Hg What mass of can dissolve in 1.0 L of water at 25 °C if the partial pressure of O 2 is 40 mm Hg? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 13, Problem 19PS
Textbook Problem
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## The partial pressure of O2 in your lungs varies from 25 mm Hg to 40 mm Hg What mass of can dissolve in 1.0 L of water at 25 °C if the partial pressure of O2 is 40 mm Hg?

Interpretation Introduction

Interpretation: The mass of oxygen has to be identified.

Concept introduction:

Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.

Sg= kHPg,where,Sgisthegassolubility(inmol/kg)kHis Henry's constant Pg is the partial pressure of the gaseous solute.

### Explanation of Solution

Given data:

Partial Pressure of O2 = 40 mm Hg = 40mmHg760mmHg=0.053bar

1L of water has mass 1kg.

Concentration=k×P(Henry's law)=(1.30×10-3mol/kgbar)×(0.053bar)=6.89×10-5mol/kg

Mass of oxygen can be calculated using the equation given below:

Concentration =moleofsoluteAmountofsolvent

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