7. In this experiment, after the reaction went to completion, we let the solutions sit to equilibrate the temperature in flasks A and B. If you did not do this and the gas temperature was too high (in the reaction flask A) when you measured the volume of water displaced in the reaction, would the molar volume calculated be too high or too low? Explain why. te B. Under what conditions do real gases behave most like ideal gases? Does the air in a room at room temperature (22 °C) and pressure (1 atm) behave ideally? ■. The molar volume for CO2 and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these molar volumes slightly less than the ideal molar volume, 22.4 L/mol?
7. In this experiment, after the reaction went to completion, we let the solutions sit to equilibrate the temperature in flasks A and B. If you did not do this and the gas temperature was too high (in the reaction flask A) when you measured the volume of water displaced in the reaction, would the molar volume calculated be too high or too low? Explain why. te B. Under what conditions do real gases behave most like ideal gases? Does the air in a room at room temperature (22 °C) and pressure (1 atm) behave ideally? ■. The molar volume for CO2 and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these molar volumes slightly less than the ideal molar volume, 22.4 L/mol?
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter9: The Gaseous State
Section: Chapter Questions
Problem 75AP
Related questions
Question
![7. In this experiment, after the reaction went to completion, we let the solutions sit to equilibrate the
temperature in flasks A and B. If you did not do this and the gas temperature was too high (in the
reaction flask A) when you measured the volume of water displaced in the reaction, would the molar
volume calculated be too high or too low? Explain why.
te
B. Under what conditions do real gases behave most like ideal gases? Does the air in a room at room
temperature (22 °C) and pressure (1 atm) behave ideally?
■. The molar volume for CO2 and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these
molar volumes slightly less than the ideal molar volume, 22.4 L/mol?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c27c061-d16a-4075-8bdf-3e6d2b43249c%2F052d4cbd-5d6f-4cc9-8a95-b64c1d936102%2Facdjvsx_processed.jpeg&w=3840&q=75)
Transcribed Image Text:7. In this experiment, after the reaction went to completion, we let the solutions sit to equilibrate the
temperature in flasks A and B. If you did not do this and the gas temperature was too high (in the
reaction flask A) when you measured the volume of water displaced in the reaction, would the molar
volume calculated be too high or too low? Explain why.
te
B. Under what conditions do real gases behave most like ideal gases? Does the air in a room at room
temperature (22 °C) and pressure (1 atm) behave ideally?
■. The molar volume for CO2 and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these
molar volumes slightly less than the ideal molar volume, 22.4 L/mol?
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Recommended textbooks for you
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Principles of Modern Chemistry](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
![Chemistry: An Atoms First Approach](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry for Engineering Students](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
![Chemistry for Engineering Students](https://www.bartleby.com/isbn_cover_images/9781285199023/9781285199023_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:
9781285199023
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning