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Chemistry
OpenStudy (anonymous):

What conditions cause deviations from the "ideal" gas? Select all that apply. low temperatures high temperatures low pressure high pressure What conditions cause deviations from the "ideal" gas? Select all that apply. low temperatures high temperatures low pressure high pressure @Chemistry

8 years ago
OpenStudy (anonymous):

High pressure and low temperatures.

8 years ago
OpenStudy (anonymous):

Thanks so much I have been stuck on this for awhile. I have a test tomorrow and need some questions answered... Can you answer them for me?

8 years ago
OpenStudy (anonymous):

I can try, post them :)

8 years ago
OpenStudy (anonymous):

1 atm = _____ 1 mm Hg 14.7 mm Hg 76 mm Hg 760 mm Hg

8 years ago
OpenStudy (anonymous):

760 mmHg

8 years ago
OpenStudy (anonymous):

1. diffusion 2. phase equilibrium 3. Boyle's Law 4. solid particles 5. kinetic energy intermingling of one substance in another inverse relationship between volume and pressure vibrate only rate of condensation = rate of evaporation energy of motion

8 years ago
OpenStudy (anonymous):

Diffusion = intermingling of one substance in another Phase Equilibrium = rate of condensation = rate of evaporation Boyle's Law = inverse relationship between volume and pressure Solid Particles = vibrate only Kinetic Energy = energy of motion

8 years ago
OpenStudy (anonymous):

Thanks.

8 years ago
OpenStudy (anonymous):

The pressure of an enclosed gas depends on: the number of molecules in a unit volume and their average kinetic energy its chemical composition the altitude about sea level the number of atoms per molecule all of the above

8 years ago
OpenStudy (anonymous):

Boyle's Law represents the relationship of volume as pressure is changed. What are the variables of Boyle's Law? pressure and number of molecules of gas volume and temperature pressure and temperature volume and number of molecules of gas pressure and volume

8 years ago
OpenStudy (anonymous):

Enclosed gas question = all of the above

8 years ago
OpenStudy (anonymous):

Boyle's Law: pressure and volume

8 years ago
OpenStudy (anonymous):

Thanks again.

8 years ago
OpenStudy (anonymous):

No problem.

8 years ago
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