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Relating Translational KE and T

Why real gase...

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Why real gases which are the actually existing gases obey gas equation only under 2 conditions Low pressure High temperature

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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 behaviour of a real gas is usually depicted by plotting compressibility factor

Z

versus pressure

P

at a constant temperature. At high temperature and pressure,

Z

is usually more than one. This fact can be explained by Van der Waals' equation when :

Q. Consider the following statements.
Statement-1: The gas which follows the ideal gas equation at all ranges of temperature and pressure is called real gas.
Statement-2: All gases follow ideal gas equation at high pressure and low temperature.
Now, choose the correct option.

Q. Under what condition real gases obey ideal gas behaviour?

Which of the following represent the suitable conditions for the liquefaction of gases?

(a) low temperature, low pressure (b) high temperature, low pressure

(c) low temperature, high pressure (d) high temperature, high pressure

Assertion: Gasses obey Boyle's law at high temperature and low pressure only.

Reason: At low pressure and high temperature, gasses would behave like ideal gases.

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Relating Translational KE and T

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