500.0 liters of a gas are prepared at 700.0 mmHg and 200.0 C. The gas is placed into a tank under high pressure. When the tank cools to 20.0 C, the pressure of the gas is 30.0 atm. What is the volume of the gas?

1 Answer
Jul 29, 2017

Answer:

The key to answering this question is to know that #1*atm# pressure will support a column of mercury that is #760*mm# high...I gets a final volume of approx. #10*L#.

Explanation:

And thus #760*mm*Hg-=1*atm#

The combined gas equation tells us that #(P_1V_1)/T_1=(P_2V_2)/T_2# given a constant molar quantity of gas.

So we solve for #V_2#, where #V_2# is conceived to be the volume of the tank.....

#V_2=(P_1V_1)/T_1xxT_2/P_2#, and we immediately see (do we?) that we gots units of volume.........

#V_2=((700*mm*Hg)/(760*mm*Hg*atm)xx500*L)/(473.15*K)xx(293.15*K)/(30*atm)~=10*L#