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....

Related questions
See all questions in Atmospheric Pressure
Impact of this question
5593 views around the world
You can reuse this answer
Creative Commons License