In a gas mixture, which component will have the higher partial pressure- -the one with the higher mole number or the one with the larger molar mass?
Added by Tracy G.
Step 1
** Show more…
Show all steps
Your feedback will help us improve your experience
Shoukat Ali and 66 other Physics 101 Mechanics educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
The total pressure in a mixture of gases is equal to the partial pressure(s) of the gas with the highest molecular weight. the gas with the smallest number of moles. all the gases added together. the gas that occupies the largest volume. the gas with the greatest number of moles.
Ma Ednelyn L.
The total pressure in a mixture of gases is equal to the partial pressure(s) of the gas with the greatest number of moles. all the gases added together. the gas with the smallest number of moles. the gas with the highest molecular weight. the gas that occupies the largest volume.
Jennifer H.
Exactly equal amounts (in moles) of gas A and gas B are combined in a 1-L container at room temperature. Gas B has a molar mass that is twice that of gas A. Which statement is true for the mixture of gases and why? a. The molecules of gas B have greater kinetic energy than those of gas A. b. Gas B has a greater partial pressure than gas A. c. The molecules of gas B have a greater average velocity than those of gas A. d. Gas B makes a greater contribution to the average density of the mixture than gas A.
Recommended Textbooks
University Physics with Modern Physics
Physics: Principles with Applications
Fundamentals of Physics
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD
