# 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?

Dec 12, 2016

${P}_{2} \cong 6 \cdot a t m .$
${P}_{1} {V}_{1} = {P}_{2} {V}_{2}$ at $\text{constant temperature}$.
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 $1 \cdot a t m$ in $m m \cdot H g$. 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.