Single Choice

The expression for compressibility factor for one mole of a van der Waal's gas at Boyle temperature is?

A$$1+\dfrac{b^2}{V(V-b)}$$
Correct Answer
B$$1+\dfrac{b^2}{V^2}$$
C$$1+\dfrac{b}{V}$$
D$$1-\dfrac{b^2}{V^2}$$

Solution

The compressibility factor for van der Waal's gases
$$Z=\dfrac{PV}{RT}=\dfrac{V}{V-b}-\dfrac{a}{RTV}$$ ……….$$(1)$$
at Boyle's temperature $$T=\dfrac{a}{Rb}$$
putting in $$(1)$$
we get
$$Z=1+\dfrac{b^2}{V(V-b)}$$
Option A.

SIMILAR QUESTIONS

States of Matter - Gas and Liquid

The temperature at which a real gas obeys the ideal gas laws over a wide range of pressure is called:

States of Matter - Gas and Liquid

At moderate pressure, $$Z$$ value of gas is $$1+xp-\dfrac{yp}{T}$$. The Boyle's temperature is:

States of Matter - Gas and Liquid

The virial equation for a real gas is represented as $$ Z = 1 + \left( b - \frac { a } { R T } \right) \frac { 1 } { V _ { m } } + \left( \frac { b } { V _ { m } } \right) ^ { 2 } + \left( \frac { c } { V _ { m } } \right) ^ { 3 } + \dots $$ The Boyle temperatue for the gas is

States of Matter - Gas and Liquid

The temperature at which a real gas obeys the ideal gas laws over a wide range of pressure is called:

States of Matter - Gas and Liquid

At Boyle temperature:

States of Matter - Gas and Liquid

The temperature at which the second virial coefficient of a real gas is zero is called :

States of Matter - Gas and Liquid

Pressure remaining the constant, the volume of a given mass of ideal gas increases for every degree centigrade rise in temperature by a definite fraction of its volume at:

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