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30 December, 07:51

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?

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  1. 30 December, 10:04
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    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
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