A gas system has an initial pressure of 5590 torr with the volume unknown. When the pressure changes to 4.29 atm the volume is found to be 10.4 L What was the initial volume in mL?

Answer 1

P1 = 5590 torr

V1 = ?

P2 = 4.29 atm x 760 torr/atm = 3260 torr

V2 = 10.4 L

Assuming constant temperature (Boyles Law) we have...

P1V1 = P2V2 and solving for V1 we have...

V1 = P2V2/P1 = (3260 torr)(10.4 L)/5590 torr

V1 = 6.07 L

(NOTE: pressure decreased so the volume must increase, which it did in going from 6.07 L to 10.4 L)