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.)

Question

Want to see more full solutions like this?

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

Want to see more full solutions like this?

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

Students have asked these similar questions

Humidity is the percentage of partial pressure of water in air over the total possible water in the air. On the first day of the spring semester the humidity was 72%, but it did not feel humid outside. Calculate the partial pressure of water in air at this time and justify why it did not feel humid. You may find it helpful to compare the first day of the spring semester to the first day of the fall semester, where the humidity was 89% on the first day of class.

The decomposition of 30.354 g of potassium chlorate yields solid potassium chloride and oxygen gas that is collected at 27.05°C and a pressure of 1.075 atm. The value for the gas constant, R, is 0.08206 L•atm/mol•K. Write a balanced equation for the reaction. What volume of oxygen gas is collected in this decomposition reaction? What mass of potassium chlorate needs to decompose in order to produce 11.889 L of oxygen gas collected at the same temperature and pressure as the original experiment?

The atmosphere is a highly complex gaseous mixture that sustains life on Earth. Approximately 99% of the air is composed of nitrogen (N2) and oxygen (O2). The remaining 1% is made up of a variety of other gases, including carbon monoxide (CO), hydrogen (H2), and ammonia (NH3), among many others. Because most of the gases that comprise the atmosphere are present at very low levels (<0.002%), their quantities are often expressed in parts per million (ppm) or parts per billion (ppb) rather than as a percent. Ozone (O3) is found in the troposphere at 2.5×10−6%. Convert this value to parts per million. [O3]= _______ ppm The atmosphere contains 2.9×10−7%2.9×10−7% nitrogen dioxide (NO2). Convert this value to parts per billion. [NO2]= _______ ppb Atmospheric methane (CH4) is present at 1983 ppb. Convert this value to a percentage. [CH4]= _______ %

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

Want to see more full solutions like this?

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

Want to see more full solutions like this?

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

Want to see more full solutions like this?

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

Videos

Answer to Problem 1PS

Explanation of Solution

Want to see more full solutions like this?

Chapter 20 Solutions