# A rigid plastic container holds 1.00 L methane gas at 650 torr pressure when the temperature is 20.9°C. How much more pressure will the gas exert if the temperature is raised to 44.1°C?

${P}_{2} = 701.3 \cdot m m \cdot H g$
Well, old $\text{Charles' Law}$ holds that ${P}_{1} / {T}_{1} = {P}_{2} / {T}_{2}$ given constant volume, and constant quantity of gas, the which is the scenario we have here...we use $\text{absolute temperature}$....we ALSO know (or should know) that $1 \cdot a t m$ will support a column of mercury that is $760 \cdot m m$ high...i.e. $1 \cdot a t m \equiv 760 \cdot \text{mm Hg}$
${P}_{2} = {P}_{1} / {T}_{1} \times {T}_{2} = \frac{\frac{650 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t {m}^{-} 1}}{294.05 \cdot K} \times 317.25 \cdot K = 0.923 \cdot a t m$
...approx. $701.3 \cdot m m \cdot H g$...