Asked by Barb
A scuba diver 60 ft below the ocean surface inhales 55.0 mL of compressed air from a scuba tank at an initial pressure of 2.60 atm and temperature of 8 ∘C.
What is the final pressure of air, in atmo-spheres, in the lungs when the gas expands to 155.0 mL at a body temperature of 37 ∘C, and the amount of gas remains constant?
2.60*55/281=P2*155.00/310= 1.268 which is not correct can someone please lead me in the right direction?
What is the final pressure of air, in atmo-spheres, in the lungs when the gas expands to 155.0 mL at a body temperature of 37 ∘C, and the amount of gas remains constant?
2.60*55/281=P2*155.00/310= 1.268 which is not correct can someone please lead me in the right direction?
Answers
Answered by
DrBob222
It is correct if you punch in the right numbers. Your set us is right; the answer is wrong.
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