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Different States of Matter

Ideal gases a...

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Ideal gases and real gases are compressible or not compressible what is the compressible factor for real gases and ideal gases.

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Q. Assertion :Compressibility factor

(Z)

for non-ideal gases is at greater than

1

. Reason: Non-ideal gases always exert higher pressure expected.

The gases which strictly follow the general equation

(P V = n R T)

are called ideal or perfect gases. Actually, there is no gas which is perfect or ideal. A real gas is one which actually exists, whether it obeys gas laws strictly or not. Under ordinary conditions, only those gases nearly behave as ideal or perfect which have very low boiling points such as nitrogen, hydrogen, etc. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviations.
A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor

(Z)

Z = \frac{P V}{n R T}

Z = 1

, for ideal gases.
(ii)

Z \neq 1

, for real gases.

The unit of the compressibility factor is:

Q. Assertion :At Boyle's temperature, the compressibility factors of a gas approaches unity. Reason: At Boyle's temperature the real gases obey ideal gas laws.

Q. The compressibility factors for 1 mole of real gases at low pressure, high pressure and that of gases of very low molar masses are

Z_{1}, Z_{2}

Z_{3}

Question 5

Why are gases compressible but not liquids?

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