Question

What is the pressure of 5.0 mol nitrogen gas in a 2.0 L container at 286 K

Answer 1

The "Ideal Gas Law Equations" is 
$PV=nRT$
P= Pressure (in Pascals)
V=Volume (in Liters)
n=amount, or number (in moles)
R= 8.3145 $\frac{Pascals*Liters}{Moles*Kelvin}$ or $\frac{PaL}{molK}$
T= Temperature (In Kelvin)

$P= \frac{nRT}{V}$

Plug into the equation and you're good!
$P=\frac{nRT}{V}$
$P =\frac{(5mol)(8.3145)(286K)}{2L}$
$P=5944.8675Pa$

If your teacher cares about sig figs,
2 sig figs (significant figures)
$P=5900Pa$

For other units of pressure,
1 atm = 760 mmHG = 760 Torr = 101326 Pa = 1.01325 bar