The+Ideal+Gas+Equation

=The Ideal Gas Law Equation- by AA=

Some call me a loner. Some call me misguided. A rare amount of others have attempted to extend upon my radical beliefs. Too many have underestimated me. But on this Wiki chapter, at least, they call me the lone wolf, on the hunt, on a mission. I suppose this is who I am destined to be, seeing as my personality leads me to these selfish ends. In short, I have brought this ignominious end upon myself, and therefore I do not wish for any pity by you the reader, the person who does or does not know me, over this self-inflicted wound. It does not matter. My only intent, in this case, is to convey the information which I was called upon to give. Enjoy... -AA
 * //A Personal Message from the author...//**

//**Creation of the Ideal Gas Law**// The ideal gas law is derived from the 3 main gas laws, Charles', Boyle's and Avogadro's. I assume that the group before me did an adequate job explaining these laws, now I will explain the connection between the 3. R is a value that can be experimentally determined from the 4 other quantatative values.

//**Gas Law-Most Common Form**// where P is pressure in atm., V is Volume in L, n is amount in Mols, and T is temperature is Kelvin. R is the universal ideal gas constant, equal to .0821 L*atm/mol*K. There are other values that R can take on depending on the desired unit, therefore when using this formula it is important to be sure that all units are in the correct form or else an incorrect value will come out of calculations. In other words, R is unit-specific. This is the ideal gas law, and although most gases deviate from this to some degree, this proves to be a useful tool in many applications. With this equation we can find any value we need to know, provided we have the other three, although this sometimes proves to be tedious work. We can also use this equation to find molar volumes, given a constant temperature and pressure, which is important in stochiometric gas conversions. For example, the molar volume of a gas at STP (273 K, 1.00 atm) is V/n=RT/P=(.0821 L*atm/mol*K * 273 K)/1.00 atm= 22.4 L/mol In short, "If you have 3 values of PV=nRT, find the 4th" (Williams 12/13/07).

We have previously proven that PV/nT=R for any gas so long as that gas is well behaved (more on that in another wiki). Therefore, as long as that gas is still a gas, we can assume that these values will always equal R. It can be concluded that: If any of these values remain constant, then they are left out of the equation. For example, if amount and temperature remain constant you can leave eliminate n's and T's from the equation, so long as one is not foolish and idiotic enough to set anything equal to R. R only works when 3 of the 4 values are known, and is basically never used in initial/final state problems. It is only placed there to prove a point that it doesn't matter what state the gas is in for P, V, n, and T, so long as it is a gas.
 * //Using the Gas Law for Initial/Final State Problems//**

Substitutions of basic equations into the gas law equation gives different equations that prove to be useful in other purposes. For example, substitution of the molar mass equation n=m/MM gives the equation (MM)PV=mRT. This allows you to find the molar mass and perhaps the identity of an unknown gas experimentally. More of these further applications will hopefully be well speculated upon in a future wiki.
 * //Gas Law Variations using Substitution//**

Information is based on the AP Chem Book and prior learnings in Honors Chem. Pictoral sources were created in Paint.
 * //Sources//**

"We all have our own laws, rules to live by. Without these there is chaos, anarchy, disorder. But we all come to realize at one point that these laws are made to be tested, to be broken, for we all know that there is no great society. In truth, often times we must count on these exceptions to the rule to keep the world civilized, and quite simply, to survive." -AA
 * //Departing Words...//**