A scuba diver takes a deep breath at the surface where the pressure is 1 atm. As the diver goes deeper underwater, how does the volume of air in their lungs change if the temperature remains constant?

Question

BlackTom AI · Accepted Answer

Consider how gas behaves when pressure changes while temperature stays constant. This is governed by Boyle's law: pressure and volume are inversely related for a fixed amount of gas. 
Option Decreases: As the diver goes deeper, ambient pressure increases above 1 atm, so the volume of gas in the lungs must shrink to keep the product P·V constant. Therefore, the volume decreases. 
Option Doubles: Doubling the pressure would halve the volume, not double it; since pressure increases with depth, volume cannot double under these conditions. 
Option Stays the same: If temperature is constant but pressure increases, the volume cannot remain unchanged according to Boyle's law; a higher pressure reduces volume. 
Option Increases: Increasing depth raises pressure, which would compress the air, not expand it; thus the volume does not increase with depth under a constant temperature scenario.

2254 CHEM 0101 SEC2010 HW 9

A scuba diver takes a deep breath at the surface where the pressure is 1 atm. As the diver goes deeper underwater, how does the volume of air in their lungs change if the temperature remains constant?

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