   Chapter 13, Problem 19PS

Chapter
Section
Textbook Problem

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

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

6

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