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The van der Waals' equation for one mole...

The van der Waals' equation for one mole may be expressed as
`V_(M)^(3)-(b+(RT)/(P))V_(m)^(2)+(aV_(m))/(P)-(ab)/(P)=0`
where `V_(m)` is the molar volume of the gas. Which of the followning is incorrect?

A

For a temperature less than `T_(C),V` has three real roots

B

For a temperature less than `T_(C),V` has three imaginary roots

C

For a temperature equal to `T_(C)` all three roots of V are real and identical

D

On increasing the temp. `(TltT_(C))`, the three roots become closer to one another

Text Solution

Verified by Experts

The correct Answer is:
b
(b) Below critical temperature a gas can be liquified.
So `V_(m)` has three real roots and identical.
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