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For one mole of a van der Waals gas when...

For one mole of a van der Waals gas when b = 0 and T = 300 K , the PV vs 1/V plot is shown below . The value of the van der Waals constant a (atm `"litre"^(2) mol^(-2)`) is

A

`1.0`

B

4.5

C

1.5

D

`3.0`

Text Solution

Verified by Experts

The correct Answer is:
C
van der Waal's equation is
`(P+ a/V^(2)) (V-b)=RT`
Given `b=0," "PV+a/V=RT`
or `PV=RT-a/V`
Comparing with `y=mx+c` intercept `c=RT` Slope `m=-a`
Slope `=(y_(2)-y_(1))/(x_(2)-x_(1))=(20.1-21.6)/(3-2)=-1.5`
`:. a=1.5`
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