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Kinetic Theory of Gases

The virial eq...

Question

The virial equation for $1$ mole of a real gas is written as:

$P V = R T [1 + \frac{A}{V} + \frac{B}{V^{2}} + \frac{B}{V^{3}} + . . . .$ to higher power of $n$ ]
Where A, B and C are known as virial coefficients. If Van der Waal's equation is written in virial form, then will be the value of $B$ :

a - \frac{b}{R T}

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b^{3}

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b - \frac{a}{R T}

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b^{2}

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Solution

The correct option is D $b^{2}$

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Similar questions

P V = R T

[1 + \frac{A}{V} + \frac{B}{V^{2}} + \frac{C}{V^{3}} + . . . . . . . to higher power of n]

1

P V = R T

1 + \frac{A}{V} + \frac{B}{V^{2}} + \frac{C}{V^{3}} + . . . . . . .

n

A, B

C

B

\frac{A}{V} + \frac{B}{V^{2}} + \frac{C}{V^{3}} +

P V_{M} = R T [A + \frac{B}{V_{M}} + \frac{C}{V_{M}^{2}} + . . .]

A, B, C, . . .

Column A	Column B
(A) High pressure	(i) $P V = R T + P b$
(B) Low pressure	(ii) $P V = R T - \frac{a}{V}$
(C) $P \to 0$	(iii) $P V = R T$
(D) Neither $a$ nor $b$ is negligible	(iv) $(P + \frac{a}{V^{2}}) (V - b) = R T$

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