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Ideal Gas and Real Gas

A real gas ca...

Question

A real gas can be considered an ideal or a perfect gas, at very high temperature and/or very low pressure.

A

True

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B

False

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Q. A gas behaves more closely as an ideal gas at
(a) low pressure and low temperature
(b) low pressure and high temperature
(c) high pressure and low temperature
(d) high pressure and high temperature.

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. At very high temperature vibrational degrees also becomes active. At such temperature an ideal diatomic gas has a molar specific heat at constant pressure

C_{P} = ?

Q. The only incorrect statement for the value of γ for NH3 gas is:(Assume ideal gas behaviour) a. γ = 7/5 at moderate temperature b. γ = 5/3 at very low temperature c. γ = 10/9 at very high temperature d. γ= 7/6 considering only 50% contributionof vibrational energ

does a real gas follows gas law at low temp. and high pressure ? why or why not ?

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