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Trailer Tires Overheating.
"basskisser" wrote in message om... Rick wrote in message link.net... Mark Browne wrote: Now you have my curiosity! I understand all gases to expand about 1/270 per degree C at room temperature. Please explain how now nitrogen and oxygen differ? This should be a good one ... but don't hold your breath waiting for a response. I am just amazed that he doesn't just look up the gas laws and see for himself. Bizarre. Bass posted this and I haven't heard from him since I answered him, so if you attempt to explain it to him maybe he will finally just go away. You apparently don't know squat about the Laws of Gases. Now, Im again telling you that the ONLY reason is that the pressure to temperature ratio is more linear. Do you refute that? If so, do tell why. Now, I suspect that you don't UNDERSTAND my answer, and that is the reason that you don't think it's correct. So, allow me to explain. The nitrogen doesn't expand as much as air, for a given temperature change. The level of scientific illiteracy in this country is frightening when you see it defended so hotly by those with the smallest armory. Rick Yes, I agree, the level of scientific illiteracy is frightening. Here you go, and Shelikoff, can you read this and comment?? There are several properties of gasses that can easily be demonstrated using liquid nitrogen. These properties include phase changes (gas to liquid, liquid to gas, and visa versa), and the temperature dependence of volume. If you have a volunteer blow up a clear balloon, you can show how a gas (oxygen) can go from gas to liquid. Oxygen has a boiling point of -180o C, so when the balloon containing oxygen from someone's breath is submerged in the liquid nitrogen the oxygen is cooled to below its boiling point and it begins to condense. There is usually some water vapor present in this balloon also- under good conditions, the water vapor will condense to liquid and then freeze, thus going through two phase changes. You can also discuss the kinetics involved in the balloons expanding when they are removed from the liquid nitrogen and begin to return to room temperature. Notice how the lighter gasses do not constrict as much since the boiling points of hydrogen and helium are both lower than that of nitrogen. You may also notice though that they will also expand a bit faster than the heavier gasses. The differences in the expansion rate becomes even more obvious if argon is available. Argon has a very small difference between the freezing point and boiling point (4o C) thus an argon filled balloon will expand very rapidly. Compare this to a breath filled balloon or a balloon filled with a gas such as ethane (95o C difference between freezing and boiling points). Rick and I just worked this out for water. In a race car tire that reaches 225 F to 250 F during normal operation, there *is* a phase change in water, from liquid to vapor. The newly introduced water vapor can add a significant component to the partial pressure composition of the tire. The only thing left here is to determine how much liquid water might be found inside a tire in different settings. Now in the temperature range of interest, operating tire temperatures, are any of the materials you mention (Nitrogen, Argon, Oxygen) undergoing any phase changes? If not, do they show any appreciable deviation from the ideal gas properties in the temperature range of interest? If not, suck it up and move on. Mark Browne P. S. You would not be doing a Jax here, would you? That is, trying to define the problem in such a narrow way as to give yourself a little wiggle room. This is not necessarily a bad thing - some us miss toying with Jax! |
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