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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)
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What state of mater obeys Boyle's law?
That Law applies to the Gas phase.
What gas law applies to the bends?
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.
Why is there a limit to the depth a diver can go?
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.
What state of matter obeys Boyle's laws?
Boyle's law applies to gases. It describes the relationship between pressure and volume, stating that at constant temperature, the pressure of a gas is inversely proportional to its volume.
Which state of matter obeys Boyle's law?
Boyle's law applies to gases. It states that at a constant temperature, the pressure and volume of a gas are inversely proportional to each other.
How do you find the density of oxygen at 1.00 bar and 10 degrees C?
You can use the ideal gas law to find the density of oxygen at 1.00 bar and 10 degrees C. First, calculate the molar volume of gas using the ideal gas law. Then, divide the molar mass of oxygen by the molar volume to find the density.
What law of gas is apply in a balloon burst into flame when placed near a lighted candle?
The law that applies in this scenario is the Ideal Gas Law. When a balloon filled with a gas bursts into flame near a lighted candle, it is due to the gas inside the balloon rapidly expanding and igniting when exposed to the heat from the flame. This reaction follows the principles of the Ideal Gas Law, which describes the relationship between pressure, volume, and temperature of a gas.
Which gas law explains why there is much carbon dioxide exchanged between alveoli as there is oxygen exchanged?
diffusion
What volume of air contains 12.7g of oxygen gas at 273 K and 1.00 ATM?
Using the ideal gas law, PV = nRT, we can calculate the moles of oxygen gas present. Then, using the molar mass of oxygen, we can find the volume of air required to contain 12.7g of oxygen gas at 273 K and 1.00 atm.
Why is the boyles law applicable only the idealgases?
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.
Does air lose heat as it moves faster?
Yes it does the gas law that applies here says increase in velocity = decrease in temperature and pressure.
Explain what is meant by the partial pressure of a gas and how it applies to respiration?
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.
