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Chapter 3: Problem 16

An ideal gas, obeying kinetic theory of gases, can be liquefied: (a) It cannot be liquefied at any \(P\) and \(T\) (b) Its pressure is more than \(P\) at a temperature less than \(T\) (c) Its temperature is more than critical temperature \(T\) (d) Its pressure is more than critical pressure \(P\)

Short Answer

Expert verified
The answer is (a). An ideal gas cannot be liquefied at any pressure \(P\) and temperature \(T\) as ideal gases can't be liquefied according to the kinetic theory of gases.

Step by step solution

01

Understand liquefaction of gases

Liquefaction of a gas happens when it is converted into a liquid state. For this transition to occur, the gas must be below its critical temperature and pressure.
02

Examine potential scenarios

Examine each situation given in the exercise options: (a) It cannot be liquefied at any \(P\) and \(T\). (b) Its pressure is more than \(P\) at a temperature less than \(T\). (c) Its temperature is more than critical temperature \(T\). (d) Its pressure is more than critical pressure \(P\). It's crucial to remember that ideal gases cannot be liquefied. However, if the gas is below its critical temperature and pressure, it could potentially be liquefied.
03

Select correct condition

Based on the information given in step 1 and 2, it is clear that the gas can potentially be liquefied if its pressure is more than the critical pressure, and if the temperature is less than the critical temperature. So none of the options gives a condition under which the gas can be liquefied, hence the correct choice is (a)

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Most popular questions from this chapter

A gas is said to behave like an ideal gas when the relation \(P V / T=\) constant. When do you expect a real gas to behave like an ideal gas? (a) When the temperature is low (b) When both the temperature and pressure are low (c) When both the temperature and pressure are high (d) When the temperature is high and pressure is low

The van der Waals equation explains the behaviour of (a) ideal gas (b) real gases (c) vapours (d) non-real gases

Expansion of a gas above inversion temperature creates (a) cooling (b) heating (c) constant temperature (d) none

Gases deviate from the ideal gas behaviour because their molecules (a) possess negligible volume (b) have forces of attraction between them (c) are polyatomic (d) are not attracted to one another

Critical temperature means above this temperature at any pressure, any gas can be (a) liquefied (b) not liquefied (c) both statements are correct (d) Solified
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