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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

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:

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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