Question

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?

Answer 1

`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.