Agas 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?

Explanation:

Given data:

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

5 structural isomers

the isomers are:

n-exane :   ch3ch2ch2ch2ch2ch3

2-methylpentane :   ch3ch(ch3)ch2ch2ch3

3-methylpentane :   ch3ch2ch(ch3)ch2ch3

2,3-dimethylbutane :   (ch3)2chch(ch3)2

2,2-dimethylbutane :   (ch3)3cch2ch3