====== Ideal Gas Law ======
===== Formula =====
  * $P$ = Pressure
  * $V$ = Volume
  * $n$ = # Particles
  * $R$ = Gas law constant (($R$ = 8.31 J mol^-1K^1 = 0.0821 L atm mol^-1K^-1 = 62.4 L torr mol^-1K^-1))
  * $T$ = Temperature **__MUST BE A UNIT WITH AN ABSOLUTE ZERO TEMPERATURE (Kelvin [K] for example)__**
$PV = nRT$

$PV = k$((k is the law's constant)) is Boyle's law, it is the only inverse relationship of the ideal gas law.
$\frac{V}{T} = k$ is Charles's law, it is a direct relationship.
$\frac{V}{n} = k$ is Avogadro's law, it is also a direct relation.
$\frac{P}{T} = k$ is Gay-Lussac's law, it is once again a direct relationship.
===== Standard Conditions (STP) =====
1 mole of __any__ gas at STP condition will have a volume equal to **22.4 L**. Standard conditions are represented by the following:
  * $P$ = 1 atm
  * $T$ = 273 K
===== Derivative Formulas =====
It isn't necessarily required to know these ones as the ideal gas law covers them.
==== Combined Gas Law ====
$\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$

This can be simplified to (depending on if certain variables are equal on both sides)
  - $\frac{P_1}{T_1} = \frac{P_2}{T_2}$
  - $P_1V_1 = P_2V_2$
  - $\frac{V_1}{T_1} = \frac{V_2}{T_2}$
==== Avogadro's Law ====
$\frac{V_1}{n_1} = \frac{V_2}{n_2}$
===== Molar Mass Shortcut =====
"Molar Mass kitty cat"
> all good cats put $dRT$ over their $P$
$M = \frac{dRT}{P}$ where $M$ is the molar mass, $d$ is the density, and $R$, $T$, and $P$ represent values from the ideal gas law.