# Question #9cb33

Feb 18, 2017

Approx. $3.5 \cdot {m}^{3}$

#### Explanation:

We assume ideality, and calculate the volume occupied by an equivalent molar quantity of Ideal Gas.

Depending on your syllabus, they probably have $\text{STP}$ $\equiv$ $1 \cdot a t m$, and $273.15 \cdot K$:

$V = \frac{n R T}{P} = \frac{\frac{4300 \cdot g}{28.05 \cdot g \cdot m o {l}^{-} 1} \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 273.15 \cdot K}{1 \cdot a t m}$

$= 3.438 \times {10}^{3} \cdot L$.

I have always these types of question abstract where they ask the VOLUME occupied by a given quantity of gas at a given temperature. This assumes a scenario where the gas is introduced to an piston that can expand against $1$ $\text{atm}$. The piston must be pretty big. Anyway, you can revise this answer depending on your given definition of $\text{STP}$.