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I seem to remember combined
Avogadro's Law with the other three gas laws to produce a slightly different combined gas law that incorporated the number of moles of gas - this way, if the mass of gas was not constant, the law would still hold true. (Something like: PV/nT = k, thus P1V1/n1T1 =
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Thanks for including the derivation, but the "physical derivation" confuses me. I'm even unsure what a physical derivation IS. Could you clarify, or provide links? I'm sure others will have similar issues.
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where p stands for pressure in atm,V for volume in litres , n is the number of moles , T is temperature in kelvin and R is a constant 0.0821 litre atm molekelvin
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I'm not sure whether or not it matters, but isn't 'k' generally used as a constant rather than 'r'? Just asking since the other gas law articles use 'k'.
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You are thinking about the ideal gas law (PV=nRT), the combined gas law only focuses on the pressure, volume, and temperature of a given gas sample.
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on
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Also, this is not a law. it's simply an equation. Why is the Title of the article "Ideal Gas Law"?
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Can someone show the derivations of
Charles', Bolton's and Lussac's Law into the Combined Gas Law?
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While I can see the possibility of relevance, i'm not entirely sure it should be included.
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I don't think it's relevant enough to be included. Removed. Don't forget
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There's a formatting error in equation (9) that needs correcting. --
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This is the correct combined gas law. Ideal gas law is PV = nRT
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P2V2/n2T2). Is this just me or is it commonly accepted?
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This is currently a proper article on a proper subject.
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Generally, yes, the constant would be represented by
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