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?

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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?

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Answer 1 · 2018-07-27T18:07:24

$P_{2} = 701.3 \cdot m m \cdot H g$ $P_2=701.3*mm*Hg$

Explanation:

Well, old $Charles' Law$ $"Charles' Law"$ holds that $\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}}$ $P_1/T_1=P_2/T_2$ given constant volume, and constant quantity of gas, the which is the scenario we have here...we use $absolute temperature$ $"absolute temperature"$ ....we ALSO know (or should know) that $1 \cdot a t m$ $1*atm$ will support a column of mercury that is $760 \cdot m m$ $760*mm$ high...i.e. $1 \cdot a t m \equiv 760 \cdot mm Hg$ $1*atm-=760*"mm Hg"$

$P_{2} = \frac{P_{1}}{T_{1}} \times T_{2} = \frac{\frac{650 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}}}{294.05 \cdot K} \times 317.25 \cdot K = 0.923 \cdot a t m$ $P_2=P_1/T_1xxT_2=((650*mm*Hg)/(760*mm*Hg*atm^-1))/(294.05*K)xx317.25*K=0.923*atm$

...approx. $701.3 \cdot m m \cdot H g$ $701.3*mm*Hg$ ...

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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?

1 Answer

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