The effects of oxygen are increased at depth so that the maximum PO2 in diving is 1.6 ATA, and this is achieved at 218 fsw breathing air, 132 fsw breathing 32% O2, and 20 fsw breathing 100% O2. This is due to the effects of Dalton's Law which states that on descent, the partial pressure of all component gases increase in the same ratio as the total pressure. this results in the creation of the elevated pO2 that causes the convulsions of O2 toxicity
(taken from http://Scuba-doc.com/o2tox.htm)
That Law applies to the Gas phase.
there are several reasons. One is the effects of nitrogen narcosis, which is when you go below 100 feet in the water, you get the effects of laughing gas. the other is caused by oxygen toxicity, which is when you are breathing pure oxygen deeper than 130 feet. These are all caused by Boyle's law, I think.
Henry's law is one of the gas laws, stating that the amount a gas dissolves in a given type and volume of liquid is proportional to the partial pressure of that gas. As pressure builds, more nitrogen and oxygen gets absorbed by the blood in the body, and it tends to get absorbed faster than it gets released, meaning that when you resurface and the pressure declines, the gas in the blood is still increased.
That is a law that applies to an ideal gas, and (as an approximation) to real gases as well.
diffusion
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
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Yes it does the gas law that applies here says increase in velocity = decrease in temperature and pressure.
Partial pressure of a gas applied to respiration is explained by Dalton's Law. It states that in every mixture of gas, each individual gas has its own pressure that makes up the total pressure of gas.
Charles' Law and other observations of gases are incorporated into the Ideal Gas Law. The Ideal Gas Law states that in an ideal gas the relationship between pressure, volume, temperature, and mass as PV = nRT, where P is pressure, V is volume, n is the number of moles (a measure of mass), R is the gas constant, and T is temperature. While this law specifically applies to ideal gases, most gases approximate the Ideal Gas Law under most conditions. Of particular note is the inclusion of density (mass and volume) and temperature, indicating a relationship between these three properties.The relationship between the pressure, volume, temperature, and amount of a gas ~APEX
Oxygen Gas
it applies for everyone who crosses the law