# For an ideal gas, how do you calculate the pressure in atm if 8.25 x 10^-2 mol occupies 174 mL at 215°C?

P=(nRT)/V=??*atm
We have been quoted the moles, $n$, the temperature, $488 \cdot K$ on the absolute scale, the volume, $0.174 \cdot L$. All we need to do is choose an appropriate gas constant. $R = 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$.
Thus, $P = \frac{8.25 \times {10}^{-} 2 \cdot m o l \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 488 \cdot K}{0.174 \cdot L}$ for an answer in atmospheres.