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Question

The compression factor (compressibility factor) for 1 mole of a van der Waals' gas at 0C and 100 atmospheric pressure is found to be 0.5. Assuming that the volume of a gas molecule is negligible, calculate the van der Waals' constant a.

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Solution

We know that,

Z=PVRT

0.5=100×V0.0821×273

V=0.112 litre

According to van der Waals' equation,

(P+aV2)(Vb)=RT for 1 mole

[100+a(0.112)2][0.1120]0.0821×273

On solving, we get a=1.253 L2mol2atm.

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