The gas in a 275.0 mL piston experiences a change in pressure from 1.00 atm to 4.85 atm. What is the new volume (in mL) assuming the moles of gas and temperature are held constant?

Answer 1

Boyles law: P1V1 = P2V2

Initial volume = V1 = 275 ml

Initial pressure = P1 = 1.00 atm

Final volume = V2 = ?

Final pressure = P2 = 4.85 atm

Plugging values into Boyles Law, we have ...

(1.00 atm)(275 ml) = (4.85 atm)(V2)

275 = 4.85 V2

V2 = 275 / 4.85

V2 = final volume = 56.7 ml