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.

Related questions
See all questions in Measuring Gas Pressure
Impact of this question
20114 views around the world
You can reuse this answer
Creative Commons License