A scuba diver that ascends to the surface too quickly can experience decompression sickness, which occurs when nitrogen that dissolves in the blood under high pressure, forms bubbles as the pressure decreases during the ascent. Therefore, an understanding of the gas laws is an important part of a scuba diver's training. In fresh water, the pressure increases by 1 atm 1 atm every 34 ft 34 ft below the water surface a diver descends. If a diver ascends quickly to the surface from a depth of 34 ft 34 ft without exhaling, by what factor will the volume of the diver's lungs change upon arrival at the surface? Assume the atmospheric pressure at the surface of the water is 1 atm 1 atm.

Question

Chemistry

Evan Graham

1 May, 05:29

A scuba diver that ascends to the surface too quickly can experience decompression sickness, which occurs when nitrogen that dissolves in the blood under high pressure, forms bubbles as the pressure decreases during the ascent. Therefore, an understanding of the gas laws is an important part of a scuba diver's training. In fresh water, the pressure increases by 1 atm 1 atm every 34 ft 34 ft below the water surface a diver descends. If a diver ascends quickly to the surface from a depth of 34 ft 34 ft without exhaling, by what factor will the volume of the diver's lungs change upon arrival at the surface? Assume the atmospheric pressure at the surface of the water is 1 atm 1 atm.

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Answers (1)

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Kelly Decker · Answer 1

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Explanation:

The pressure at 34ft is the atmospheric pressure (1 atm) plus 1 atm, because at each 34ft the pressure increase by 1 atm, so it will be 2 atm. Let's assume that the lungs will be at a constant temperature, so, by the ideal gas law:

P1*V1 = P2*V2

Where P is the pressure, V is the volume, 1 is the state at 34 ft under the water, and 2 at the water surface, where P2 = 1atm. Thus:

2*V1 = 1*V2

V2 = 2V1

Thus, the volume will change by a factor of 2, so, the volume will double.