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The real gases show deviation from ideal...

The real gases show deviation from ideal gases donot follow Boyle's law, Charles law and Avogadro law perfectly under all conditions. The deviations from ideal behaviour can be measured in terms of compressibility factor, Z which may be defined as :
`Z=(pV)/(nRT)`
It has been observed that Z has values greater than and less than one for different gases. The behaviour of some common gases is shown here.

If `V_(o)` is the observed volume of a gas and `V_(i)` is the ideal gas volume, then Z is

A

`V_(o)-V_(i)`

B

`V_(o)//V_(i)`

C

`V_(i)//V_(o)`

D

`V_(i)-V_(o)`

Text Solution

Verified by Experts

The correct Answer is:
B
`Z=(V_("real"))/(V_("ideal"))`
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