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Gay Lussac's Law

Which of the ...

Question

Which of the following is not true for gases:

A

A gas above its critical temperature can be liquefied

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B

A gas is different from a vapour

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C

All existing gases are real

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D

Ideal gas obeys all gas laws at all temperature and pressures

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Solution

The correct option is A
A gas above its critical temperature can be liquefied

A gas above its critical temperature can be liquefied

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Q. In the following statements:
(A) Ideal gases are liquefied only at very low temperatures.
(B) Ideal gases cannot be liquefied.
(C) Ideal gas behaviour is observed by real gases at low pressures.
(D) Ideal gases do not exist.
The correct statements are:

Q. Assertion (A): Real gases tend to behave as ideal gas at low pressure and high Temperature.
Reason (R): At temperature more than critical temperature, a gas can’t be liquefied just by increasing the pressure. Which of the followings is correct?

Q. The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called

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. Critical temperature and critical pressure values of four gases are given

\begin{matrix} Gas & C. Temp (K) & C. Pressure (atm) P & 5.1 & 2.2 Q & 33 & 13 R & 126 & 34 S & 135 & 40 \end{matrix}

Which of the gas/gases cannot be liquefied at a temperature of 100 K and a pressure of 50 atmospheres?

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