# If 15.0 g CO_2 gas has a volume of 0.30 L at 300 K, of what is its pressure in millimeters of mercury?

Oct 15, 2016

This is a high pressure system, whose pressure could not be reasonably measured in $\text{mm Hg}$. A pressure of $28.0 \cdot a t m$ would be developed given these parameters.

#### Explanation:

We work out the pressure in $\text{atmospheres}$ for $\frac{15.0 \cdot g}{44.0 \cdot g \cdot m o {l}^{-} 1} = 0.341 \cdot m o l$ of an Ideal Gas.

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

$\frac{0.341 \cdot m o l \times 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1 \times 300 \cdot K}{0.30 \cdot L}$

$=$ $28.0 \cdot a t m$

I suspect that the question originally proposed a $0.15 \cdot g$ mass of gas, which would lead to a pressure of less than an atmosphere, where a reading in $\text{mm Hg}$ would be reasonable.