Deep-sea divers commonly use oxygen blended with an inert gas. The partial pressure of oxygen changes according to the needed requirement. After every depth of 100 feet, the diver experiences 3 atm pressure, resulting in inability to inhale normal air. Which gas law best explains the process involved Blank 1
The gas law that best explains the process involved is the Boyle's law, which states that the pressure of a gas is inversely proportional to its volume at a constant temperature. As the diver descends deeper into the ocean, the pressure increases and the volume of the gas in their tank decreases. By blending oxygen with an inert gas, the partial pressure of oxygen can be adjusted to meet the demands of the diver at different depths.
The gas law that best explains the process involved in this scenario is Boyle's Law.
Boyle's Law states that at a constant temperature, the pressure of a gas is inversely proportional to its volume. In this case, as the deep-sea diver descends to greater depths, the pressure increases, causing the volume of the gas to decrease.
Since the diver experiences 3 atm pressure after every 100 feet, the volume of the gas (oxygen and inert gas blend) would decrease accordingly. This is why the diver is unable to inhale normal air at those depths and requires a different gas mixture to compensate for the increased pressure.