Question

A container of gas at 2.8 atm pressure and 120∘C is compressed at constant temperature until the volume is halved. It is then further compressed at constant pressure until the volume is halved again.

1.) What is the final pressure of the gas?(in atm)

2.)What is the final temperature of the gas?(in celsius)

Answer #1

Given is:-

Initital pressure of the gas = 2.8 atm , temperature = 120c or 393K

First of all it is compressed at constant temperature that means the process is Isothermal therefore the process is described by Boyle's Law:-

by putting all these values in the above equation, we get

Therefore the pressure is doubled.

Now in the second process it is further compressed at constant pressure therefore the process is described by Charle's Law:-

Let's say then

by putting all these in above equation we get

or

Therefore the final pressure of the gas is 5.6atm (Part-a)

and the final temperature of the gas is -76.5 C (Part-b)

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