In: Chemistry
A suba diver 60ft below the ocean surface inhales 50.0mL of compressed air at 3.00 atm and 241K from a scuba tank. What is the pressure of the air at 37C in the lungs where it expands to 150.mL?
Initial conditions of air:
Pressure P1 = 3.00 atm
Volume V1 = 50.0 mL
Temperature T1 = 241 K
Final conditions of air:
Pressure P2 = ?
Volume V2 = 150 mL
Temperature T2 = 37 oC = 37 + 273 K = 310 K
We know that P1V1/T1 = P2V2/T2
P2 = (P1V1/T1) (T2/V2)
= ( 3.00 atm x 50.0 mL/ 241 K ) ( 310 K/ 150 mL)
= 1.286 atm
P2 = 1.286 atm
Therefore,
Final pressure of the air = 1.286 atm