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.

1 Answer
anor277
Jun 11, 2018

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

Explanation:

And #1*atm-=760*mm*Hg# or rather #1*atm# will support a column of mercury that is #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.."# #P_1V_1=P_2V_2#

We solve for #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))#

#-=1.14*L#...the VOLUME has reduced because we INCREASED the PRESSURE....

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