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The gases which strictly follow the gene...

The gases which strictly follow the general equation `(PV = nRT)` 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 ect. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviation
A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor (Z)
`Z = (PV)/(nRT)`
(i) `Z = 1`, for ideal gases.
(ii) `Z != 1`, for real gases.
Consider the equation `Z = (PV)/(nRT)`, which of the following statements is correct ?

A

When `Z gt 1`, real gases are easier to compress than the ideal gas

B

When `Z = 1`, real gases get compressed easily

C

When `Z gt 1`, real gases are difficult to compress

D

When `Z = 1`, real gases are difficult to compress

Text Solution

Verified by Experts

The correct Answer is:
C
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The gases which strictly follow the general equation (PV = nRT) 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 ect. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviation A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor (Z) Z = (PV)/(nRT) (i) Z = 1 , for ideal gases. (ii) Z != 1 , for real gases. The units of compressibility factor are :

The gases which strictly follow the general equation (PV = nRT) 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 ect. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviation A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor (Z) Z = (PV)/(nRT) (i) Z = 1 , for ideal gases. (ii) Z != 1 , for real gases. At low pressure, the van der Waals' equation is reduced to :

The gases which strictly follow the general equation (PV = nRT) 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 ect. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviation A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor (Z) Z = (PV)/(nRT) (i) Z = 1 , for ideal gases. (ii) Z != 1 , for real gases. At Boyle's temperature, compressibility factor Z for a real gas is :

The gases which strictly follow the general equation (PV = nRT) 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 ect. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviation A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor (Z) Z = (PV)/(nRT) (i) Z = 1 , for ideal gases. (ii) Z != 1 , for real gases. The behaviour of a real gas is usually depiected 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 Waal's equation when :

Real gases do not obey ideal gas equation,

Which of the following gases behaves like are ideal gas?

Real gases behave ideally at:

All curves for real gases approach the ideal gas behaviour at