Chemistry, asked by Anonymous, 9 months ago

explain the application of Henry's law in the deep sea diving.(5 marks)​

Answers

Answered by MajorLazer017
26

Application of Henry's law in deep sea diving :

Deep - sea divers (or scuba divers) depend upon compressed air for their oxygen supply. According to Henry's law, solubilities of gases increase with pressure. Thus, both N2 and O2 will dissolve considerably in the blood and other body fluids.

Oxygen is used up for metabolism, but due to high partial pressure and great solubility, N2 will remain dissolved and will form bubbles when the diver comes to the atmospheric pressure.

These bubbles affect nerve impulses and give rise to a disease called bends or decompression sickness. To avoid bends and also the toxic effects of high concentration of nitrogen in the blood, the cylinders used by the divers are filled with air diluted with helium.

Answered by Manulal857
1

Answer:

Hey Buddy here's ur answer

The implication of this law for SCUBA diving is that as depth increases (and therefore pressure) the amount of a gas dissolved in the diver's blood will also increase. Oxygen is consumed by the body's physiological processes, but nitrogen is physiologically inert.

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