Question

In: Chemistry

A scuba diver 40ft below the ocean surface inhales 50.0 mL of compressed air from a...

A scuba diver 40ft below the ocean surface inhales 50.0 mL of compressed air from a scuba tank at a pressure of 3.50 atm and a temperature of 6 degrees celsius.

Part A: What is the pressure of the air, in atm, in the lungs when the gas expands to 150.0 mL at a body temperature of 37 degrees celsius, and the amount of gas remains constant?

Expert Solution

V₁= 50 mL

P₁= 3.50 atm

T₁= 6℃= 6+273= 279‬ K

V₂= 150 mL

P₂= ?

T₂= 37 ℃= 37+273= 310 K

since

P₁V₁/T₁= P₂V₂/T₂

therefore

P₂= P₁V₁T₂/V₂T₁

Plug in all values

P₂= 50mL*3.50 atm*310 K/150 mL* 279 K

P₂=1.30 atm

Therefore final pressure P₂=1.30 atm

Your one thumbs up will help me lot. Thanks!

queen_honey_blossom answered 2 years ago

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