Chlorine gas occupies a volume of 1.20 liters at 720 torr pressure. What volume will it occupy at 1 atm pressure? Assume that temperature remains the same.

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Chlorine gas occupies a volume of 1.20 liters at 720 torr pressure. What volume will it occupy at 1 atm pressure? Assume that temperature remains the same.

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Answer 1 · 2018-06-11T16:08:54

Well, $1 Torr = 1 mm Hg$ $"1 Torr = 1 mm Hg"$ ...

Explanation:

And $1 \cdot a t m \equiv 760 \cdot m m \cdot H g$ $1*atm-=760*mm*Hg$ or rather $1 \cdot a t m$ $1*atm$ will support a column of mercury that is $760 \cdot m m$ $760* mm$ high...and I truly hope you have seen such a column because the health and safety commissars at my establishment have declared the mercury column counter-revolutionary.

And we simply apply old $Boyles' Law..$ $"Boyles' Law.."$ $P_{1} V_{1} = P_{2} V_{2}$ $P_1V_1=P_2V_2$

We solve for $V_{2} = \frac{P_{1} V_{1}}{P_{2}} = \frac{1.20 \cdot L \times \frac{720 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}}}{\frac{760 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}}}$ $V_2=(P_1V_1)/P_2=(1.20*Lxx(720*mm*Hg)/(760*mm*Hg*atm^-1))/((760*mm*Hg)/(760*mm*Hg*atm^-1))$

$\equiv 1.14 \cdot L$ $-=1.14*L$ ...the VOLUME has reduced because we INCREASED the PRESSURE....

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Chlorine gas occupies a volume of 1.20 liters at 720 torr pressure. What volume will it occupy at 1 atm pressure? Assume that temperature remains the same.

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