# If there are 115.6*L of fluorine gas at "STP", what is the molar quantity?

May 25, 2017

Approx. $5 \cdot m o l$.................

#### Explanation:

The molar volume of an Ideal Gas at $\text{STP}$ is $22.4 \cdot L$, and thus number of moles $= \text{volume of gas"/"molar volume}$. We assume that behaviour of ${F}_{2} \left(g\right)$ approaches ideality.

$= \frac{115.6 \cdot \cancel{L}}{22.4 \cdot \cancel{L} \cdot m o {l}^{-} 1} = 5.16 \cdot \frac{1}{m o {l}^{-} 1}$

$= 5.16 \cdot \frac{1}{\frac{1}{m o l}} = 5.16 \cdot m o l$.

What is the mass of this quantity of gas?