# If an ideal gas has a pressure of 4.97 atm, a temperature of 481 K, and has a volume of 29.83 L, how many moles of gas are in the sample?

May 13, 2016

$n \cong 4 \cdot m o l$
$n = \frac{P V}{R T}$ $=$ $\frac{4.97 \cdot \cancel{a t m} \times 29.83 \cdot \cancel{L}}{0.0821 \cdot \cancel{L} \cdot \cancel{a t m} \cdot \cancel{{K}^{-} 1} \cdot m o {l}^{-} 1 \times 481 \cdot \cancel{K}}$ $=$ ??*mol.
Note that the only problem in solving this problem is choosing an appropriate gas constant, $R$. For chemists, $R = 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$, is very useful because it uses the units that chemists would typically use, i.e. $\text{atmospheres, litres, etc.}$. Is the equation correct dimensionally?