# What pressure (in atm) will 0.44 moles of CO_2 exert in a 2.6 L container at 25°C?

Oct 30, 2016

P=(nRT)/V=??*atm
$P = \frac{0.44 \cdot \cancel{m o l} \times 0.0821 \cdot \cancel{L} \cdot a t m \cdot \cancel{{K}^{-} 1} \cancel{m o {l}^{-} 1} \times 298 \cdot \cancel{K}}{2.6 \cdot \cancel{L}}$
$=$ ?? atm.
The $\text{Gas constant}$, $R$, most generally used by chemists is $0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$. Sometimes, we use ${\mathrm{dm}}^{3}$, i.e. $1 \cdot {\mathrm{dm}}^{3} = {\left(1 \times {10}^{-} 1 \cdot m\right)}^{3} = {10}^{-} 3 \cdot {m}^{3}$, i.e. $1 L = 1 \cdot {\mathrm{dm}}^{3} = {10}^{-} 3 {m}^{3}$.