Henry’s Law

Henry’s Law occurs when one is scuba diving. When a scuba diver is at a deeper depth, there is more pressure being exerted on the diver. This causes the air the diver is breathing, out of the scuba tank, to be compressed air. The air we breathe is aobut 80% nitrogen and 20% oxygen. As one scuba dives, the partial pressure of nitrogen and oxygen increases. Oxygen has to be at a much higher partial pressure to infilict harm to you. On the other hand, nitrogen does not pose a threat. Henry’s Law states that gasses have the ability, under pressure, to dissolve into a liquid. Henry’s Law explains why some scuba divers develop “the bends.” Henry’s Law relates to Dalton’s Law. Henry’s Law relates to Dalton’s Law because, the partial pressure of nitrogen dissolved into the scuba diver’s body at depth effects if they develop The Bends. Henry’s Law also explains how a gas can be released from a liquid in the form of bubbles. A daily example of this is a soda bottle, when the bottle is opened the pressure decreases causing bubbles to emerge from the liquid.


Dive Table

Decompression Sickness

When divers surface too fast, after being at a depth where the partial pressure of nitrogen is very high, they can develop nitrogen bubbles in the bloodstream or tissues. Decompression sickness can be treated by going to a Decompression Chamber. The Decompression Chamber re-pressurizes the diver back to certain depths for the proper amount of time to allow the nitrogen to be released via the lungs when one exhales. In the worst possible case, decompression sickness can result in unconsciousness or even death.

Chemical Sciences. Henry's Law and the solubility of gases.

Henry's Law