# What is the molar volume of 5.00 moles of bromine gas?

Jun 10, 2014

We can only calculate this value if we assume the gas is at standard temperature and pressure, based upon the information you have provided.

There are two ways to calculate this if we assume STP of 1 atm and 273 K for the pressure and temperature.

We can use the Ideal Gas Law equations PV = nRT
P = 1 atm
V = ???
n = 5.00 moles
R = 0.0821 $\frac{a t m L}{m o l K}$
T = 273 K

$P V = n R T$ can be $V = \frac{n R T}{P}$

$V = \left(\frac{\left(5.00 m o l\right) \left(0.0821 \frac{a t m L}{m o l K}\right) \left(273 K\right)}{1 a t m}\right)$

#V = 112.07 L

The second method is to us Avogadro's Volume at STP $22.4 L = 1 m o l$

$5.00 m o l x \frac{22.4 L}{1 m o l} = 112 L$