The pressure in the air in a scuba diver’s lungs when she is 15m un derwater is

Question

The pressure in the air in a scuba diver’s lungs when she is 15m un derwater is 2.5x10 5 N/m 2 (equal to the pressure of the water at that depth), and the air occupies a volume of 4.8 L. Assume air is like an ideal gas, and that the number of moles in the lung s do not change (until part c). a) What is the volume of the air in the diver’s lungs when she reaches the surface, where the pressure is 1.0x10 5 N/m 2 ? Assume the gas temper ature is 37°C. b) How many moles of gas are in the diver’s lungs? c) How many moles should she exhale so that the final volume of gas is only 6L (this is at the surface).

Explanation / Answer

(a) PV = constant

(2.5 x 10^5) (4.8L) = (1 x 10^5) (V)

V = 12 L

(B) P V = n R T

(2.5 x 10^5) (4.8 x 10^-3 m^2) = n (8.314)(273+37)

n = 0.466 mol

(c) (1 x 10^5) (6 x 10^-3) = n' = (8.314) (273 + 37)

n' = 0.233 mol

mole exhale = n - n' = 0.233 moles

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