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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

In the discussion on the composition of air, mention is made of the fact that water vapor may have a concentration as high as 40,000 ppm. Calculate the partial pressure exerted by water vapor at this concentration. Assume that this represents a situation with 100% humidity. What temperature would be needed to achieve this value? (See Appendix G.)

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000ppm concentration and the temperature which is needed to achieve the calculated partial pressure should be determined.

Concept introduction:

  • Parts per million (ppm) concentrations: It is the ratio of the number of grams of solute for every one million grams of solution.

 Partspermillion(ppm) =MassofsoluteMassofsolution×106

For gases, ppm refers to numbers of particles and hence to mole fraction. And the gas pressure exerted is directly proportional to the mole fraction.

Explanation

For gases, ppm refers to numbers of particles and hence to mole fraction. And the gas pressure exerted is directly proportional to the mole fraction.

The pressure exerted by water vapor at 40,000ppm concentration is,

    400001000000ofoneatmosphere0

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