Can anyone explain postulate gases?
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You can find a good summary here:\n\nhttp://www.sparknotes.com/testprep/books/sat2/physics/chapter12section2.rhtml
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Any gas (CO2, N2, whatever) that doesn't abide by the Ideal Gas Law....\n\nIDEAL gases are just that, IDEALS, and they abide by PV=nRT.\n \nIn the real world, gases abide by a more modified version of this equation.  Hence the term, "real" gases.
413674
Some of the elements while in gaseous state.
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Here's a great website with pictures of the various nobel gases in lamps so you can see their glows and describe them yourself.\n\nhttp://www.assumption.edu/users/bniece/Spectra/Complete.html
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How very astute.  Fluids form mixtures and circulate based on different things, like pressure and heat.\n\nBut the gases do form layers.  Who said they don't?
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You get napalm.\n\nIf you google "gasoline and styrofoam", the first thing that pops up is a short explanation from totse.com which has a TON of other articles about things like this.
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You might want to try to re-read the questions.  You don't appear to be understanding what is written there.  (I call it a brain fart, but three out of 28 indicates a little lack of understanding)\n\nIf you have re-read the problems, then I offer the below:\n\nYou might want to go over your notes about what a mole is.  It is an amount and a number.  It is a fundamental conceptual building block for the study of chemistry.\n\n  It looks like you expect to be able to plug and chug on these.  Which you can, once you start thinking in terms of atoms and molecules.  Plugging and chugging BEFORE you understand what these little pieces are doing is a recipe for a C.\nIt IS the ATOMIC theory of matter, don't you know.\n\nSo, once you've absorbed that, re-read these three problems.\n\nStill no joy?  Read on, Gunga DIn\n\nFirst H(g) is NOT the element's standard state! I thought everybody learned in grade school about H2 gas - the simplest molecule?  Iodine, I leave to you  (hint a gas???!!! not)\n\nSecond lets see you're making umpteen moles of something and calculate the dS.  that was not the question.  (hint: something about ONE mole)\n\nThird read the problem. your chemical equation is from I don't know where but not from what is in the problem. (hint: products on the LEFT???)
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postulates are geometric concepts that we accept as true. Theorems must be deductively proven as true.  The problem is, what one geometry book offers as a postulate, another book may have as a theorem.\n\nSee your geometry teacher for some extra help, that's what the teacher is there for. Good luck.
1135127
Since SO2 is symmetrical with the outer oxygen atoms bound at 180 degrees, I don't believe it has a dipole moment.  O3 is the same, having the oxygens on the outside, so there is no "pole," and although there is a slight 30-degree "kink" to CS2, I don't believe it has a dipole either.  I believe you need to actually have hydrogen present for a hydrogen bond to occur... these are all gases, and are therefore not bound to anything in this gaseous form.
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gas cools down if it expands suddenly.\n\nsimilar principle is used in AC and refrigerators.
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Ideal gas laws assume that all particles are spherically symmtric and engage only in elastic collisions.  They ignore all other types of molecular energy (rotation in other planes of symmetry or asymmetry, bond stretching/compressing/bending, rotation about a molecular bond--all these things can and do absord energy from a collision), and they negate the effects of all intermolecular forces, like dipole interations, hydrogen bonding, London dispersion forces, etc.\n\nIn gases like helium, the atoms are basically spherically symmetric, and most of these random forces are neglible.  Hence, ideal gas laws work really well for these--only at really ridiculously low temperatures and high pressures do these forces manage to liquify helium.  The larger you molecule is--and I'm not talking about mass so much as the number of chemical bonds--the less ideally it behaves.  The greater the heterogeneity of a gass, the less ideally it behaves.  The greater the polarity (eg seperation of charges) displayed by the molecule, the less ideally it behaves.
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sky is nothing but made up of gases . as gases rise uo they all collect above
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the actual equation is:  (p + b·n^2/V^2)(V - a·n) = nRT\n\na:- every mol of particles of the gas has a tiny finite volume of a\n\nb:-modification is due to the particles sticking to each other, a phenomenon called cohesion\n\nR- rydberg's constant
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Yup!\n\nThe gas is colorless, odorless, and tasteless. The liquid and solid forms are a pale blue color and are strongly paramagnetic.
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Hey Dude! Do you know how many different types of gases there are!!!! Do you! I can't even list all the types of gases here! Jeez!
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Use the gas law\nPV=nRT
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This ain't my forte, but here goes.\n\nAdiabatic expansion is like what my freezer and air conditioner use to cool things off.  They take a pressurized gas and let it expand, which drops its temperature.  Then they let this low-temperature stuff suck up the heat in my Ben & Jerry's or in my house.  If you've ever discharged a CO2 fire extinguisher or used a can of compressed air to clean your computer, the CO2 is so cold it condenses the water in the atmosphere or the air on your computer is very cold.\n\nIsothermal means the temperature stays the same.  So if your gas expanded and it didn't get colder, something else went on to provide the heat to keep the temperature the same.  \n\nMaking heat is work, in physics terminology, so the isothermal expansion required more work than the adiabatic expansion.