A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

1 Answer
anor277
Dec 12, 2016

#P_2~=6*atm.#

Explanation:

#P_1V_1=P_2V_2# at #"constant temperature"#.

#P_2=(P_1V_1)/V_2=(946*cancel(mL)xx(726*cancel(mm*Hg))/(760*cancel(mm*Hg)*atm^-1))/(154*cancel(mL))=??atm#

Note that you do NOT measure a pressure that is over #1*atm# in #mm*Hg#. You do this and you will get mercury all over the laboratory. It's a big deal and a big, messy clean up job if you spill it.

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