A gas with constant temperature has a pressure of 4 atm. This pressure changes to 0.2 atm, causing the volume to increase to 500 L. Based on the relationship between pressure and volume, what must have happened to the pressure?

Given dа ta:

Initial pressure P1 = 4 atm

Final pressure P2 = 0.2 atm

Final volume V2 = 500 L

Solution:

First of all we will calculate the initial volume of gas.

P1V1 = P2V2

V1 = P2V2 / P1

V1 = 0.2 atm * 500 L / 4 atm

V1 = 25 L

We can see that in given problem as the volume is increases from 25 L to 500 L pressure is goes to decrease from 4 atm to 0.2 atm.

According to the boyle's law, The volume of given amount of gas is inversely proportional to its pressure, at constant temperature.

V∝ 1/p

V = K/P

PV = K

so,

P1V1 = K and P2V2 = K

or

P1V1 = P2V2