# How can I calculate the volume, in liters, of 1.50 mol Cl2 at STP?

May 25, 2014

To calculate this we can use the Ideal gas law of $P V = n R T$

At STP (Standard Temperature and Pressure)
P = 1 atm
V = ?
n = 1.50 mol
R = 0.0821 $\frac{a t m L}{m o l K}$
T = 273 K

$\left(1 a t m\right) \left(V\right) = \left(1.50 m o l\right) \left(0.0821 \frac{a t m L}{m o l K}\right) \left(273 K\right)$

$V = \frac{\left(1.50 m o l\right) \left(0.0821 \frac{a t m L}{m o l K}\right) \left(273 K\right)}{1 a t m}$

$V = 33.6 \frac{L}{m} o l$