Knowledge to share with

Haha!!:yesterday night was a miracle! what a finally I get my study mood back..Haha! Yea..you dunno how happy i am last night..kind of sad i can't share it out yesterday, but nvm la~it is quite impossible for you all get the info which same with mine while i'm sleeping right?Muahahaha!!!

OK ok!! yesterday discover this, we study three gas law when we were all in Form 5 last year (2010) but yesterday erad on book and find out the real three gas law is Boyle's law, Charles and Gay-Lussac's Law (normally named as Charles's Law) and the last one is no more Archimedes's law but Avogadro's Law..surprise right?^^
ok la..briefly explain Boyle's and Charle's..formula for Boyle's VP=k, formula for Charles's V/T = k..
Avogadro's law, which states that at constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of the gas present. that's the defination. understand bor? if not just refer to the formula below , V/n = k...the 'k' stands for proportionality constant..which later will be replace with capital letter of r, 'R'. ok. ..short enough ==

main thing is actually not the three law but the "Ideal Gas Equation" it is used to calculate all the gas de thing lor..it's formula, actually is the combine of the three gas laws stated above just now..so its formula is actually like this
V is directly proportional to nT/P
V = R(nT/P)
or PV = nRT
key word, P = Pressure
V= Volume
n = number of mole

the defination : describes the relationship among the four variables P, V, T, and n. And ideal gas is a hypothetical gas whose pressure-volume-temperature behavior can be completely accounted for by the ideal gas equation.  the molecules of an ideal gas do not attract or repel one another, and their volume is negligible compared with the volume of the container.  although there is no such thing in nature as an ideal gas, discrepancies in teh behavior of real gases over reasonable temperature and pressure ranges do not significantly affect calculations.  thus we can safely use the ideal gas equation to solve many gas problems..

so ok?i  continue with the text har...haha~:DD

P/S: take the * as degree, since i dun have the symbol here==

before we can apply the ideal gas equation to a real system, we must evaluate the gas constant R.  At 0*C (273.15K) and 1 atm pressure, many real gases behave like an ideal gas.  experiments show that under thes conditions, 1 mole of an ideal gas occupies 22.414L, which is somewhat greater than the volume of a basketball...The condition 0*C and 1 atm are called standard temperature and pressure, often abbreviated STP


ok la..i think i will stop here..or else u will get bored till the maX!!haha..i dunno how much of u will read it till the end..but at least i hope it will help at least a little in your future xDD~good luck~