Chapter 13, Problem 19PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
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:

PartialÂ PressureÂ ofÂ O2Â =Â 40Â mmÂ HgÂ =Â 40mmHg760mmHg=â€‰0.053bar

1L of water has mass 1â€‰kg.

Concentrationâ€‰â€‰=â€‰â€‰â€‰kÃ—P(Henry'sÂ law)â€‰â€‰â€‰=â€‰â€‰(1.30Ã—10-3mol/kgâ€‰bar)Ã—(0.053bar)â€‰â€‰â€‰=â€‰â€‰â€‰6.89Ã—10-5mol/kg

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

ConcentrationÂ =â€‰â€‰moleâ€‰ofâ€‰soluteAmountâ€‰ofâ€‰solvent

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