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If two gases have same value of $a$ but different values of b (a and b are van der Waal's constant) which of the following statement is wrong ?

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The gas having smaller value of $b$ has larger compressibility

The gas having smaller value of b will occupy lesser volume

The gas having smaller value of $b$ has lesser compressibility

Both (a) and (b)

answer is C.

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Detailed Solution

The gas molecules' effective size is represented by the value of $b$ . Smaller size and more compressible volume are indicated by a smaller value of $b$ .

As a result, the gas will be more compressible if $b$ is less.

So, option C is correct.

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