The average kinetic energy of an ideal gas molecule is (KE) = kpT (a) Air is mostly diatomic nitrogen. Use the above formula to calculate the average velocity of an air molecule at room temperature (300 K). [m/s]
The average kinetic energy of an ideal gas molecule is (KE) = kpT (a) Air is mostly diatomic nitrogen. Use the above formula to calculate the average velocity of an air molecule at room temperature (300 K). [m/s]
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![1. The average kinetic energy of an ideal gas molecule is
(KE) = kBT
(a) Air is mostly diatomic nitrogen. Use the above formula to calculate the average velocity
of an air molecule at room temperature (300 K). [m/s]
(b) I have a 1 m long cylinder, which I compress with a piston to 0.5 m steadily over 10
seconds. Based on your answer to (a), can I consider this an "adiabatic" process?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5edf3b93-3aff-4c16-90eb-deaa12bfa77c%2F51a47b58-ada8-4d40-b89b-925897e3f905%2Fur0kvoj_processed.png&w=3840&q=75)
Transcribed Image Text:1. The average kinetic energy of an ideal gas molecule is
(KE) = kBT
(a) Air is mostly diatomic nitrogen. Use the above formula to calculate the average velocity
of an air molecule at room temperature (300 K). [m/s]
(b) I have a 1 m long cylinder, which I compress with a piston to 0.5 m steadily over 10
seconds. Based on your answer to (a), can I consider this an "adiabatic" process?
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