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.)

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Answer 1

Textbook Question

Chapter 20, Problem 1PS

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.)

Expert Solution & Answer

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Conclusion

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

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Answer 2

Textbook Question

Chapter 20, Problem 1PS

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.)

Expert Solution & Answer

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Conclusion

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

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Textbook Question

Chapter 20, Problem 1PS

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.)

Expert Solution & Answer

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Conclusion

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

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Textbook Question

Chapter 20, Problem 1PS

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.)

Expert Solution & Answer

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Conclusion

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

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution & Answer

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Conclusion

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

Answer 8

Expert Solution & Answer

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Conclusion

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

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Interpretation Introduction

Interpretation:

The partial pressure exerted by water vapor at 40,000 ppm 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.

Parts per million (ppm)= Mass of soluteMass of solution ×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.

Answer 12

Answer to Problem 1PS

The partial pressure exerted by water vapor at 40,000 ppm concentration is 30.4 mmHg.

Answer 13

Explanation of Solution

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 40,000 ppm concentration is,

400001000000 of one atmosphere ≅ 0.04 ×760 mmHg = 30.4 mmHg

This pressure partial pressure can be achieved if the temperature value reaches above 29 0C.

Answer 14

Conclusion

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

Answer 15

Ch. 20.1 - Prob. 1RC Ch. 20.1 - Prob. 2RC Ch. 20.2 - Prob. 1RC Ch. 20.2 - Prob. 2RC Ch. 20.3 - Prob. 1RC Ch. 20.3 - Prob. 2RC Ch. 20.3 - Prob. 3RC Ch. 20.4 - Prob. 1RC Ch. 20.4 - Prob. 2RC Ch. 20.4 - 3. Which of the following is a renewable energy...

Solution Summary: The author explains the partial pressure exerted by water vapor at 40,000ppm concentration and the temperature which is needed to achieve the calculated partial

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