# What volume is occupied by a 2*mol quantity of oxygen, nitrogen, and fluorine gases, at 300*K under a pressure of 1.3*atm?

Sep 8, 2017

Approx. $40 \cdot L$..........

#### Explanation:

We use the old ideal gas law.....

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

We must simply KNOW that oxygen, and nitrogen, and fluorine, and chlorine, are DIATOMIC gases, i.e. ${X}_{2}$...(this is the next refinement of this problem, they could have mentioned a mass of $64 \cdot g$....)

And so.......

$V = \frac{2 \cdot m o l \times 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1 \times 300 \cdot K}{1.3 \cdot a t m}$

=??L....Do the units in the calculation cancel out to give an answer in litres? They should, and if they don't then somewhere we have made an error.