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Chapter 3: Problem 6

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

Short Answer

Expert verified
(b) real gases

Step by step solution

01

Analyze the choices

The first step is to understand each of the following options: (a) ideal gases, (b) real gases, (c) vapours, and (d) non-real gases. The ideal gas law is a hypothetical gas law that assumes gas particles do not interact and occupy no volume. Real gases are gases that do not follow the ideal gas laws exactly, due to interactions between particles and a finite volume of the particles. Vapours are a specific state of matter, not a category of gases. Non-real gases don't exist, there are only ideal and real gases in terms of behavior.
02

Match the choice with the concept of van der Waals equation

The van der Waals equation is used to understand the behavior of real gases, including their properties under different conditions. It includes terms to account for the finite volume of gas molecules and the intermolecular forces, things that ideal gases ignore. Hence, this equation doesn't apply to ideal gases, vapours, or 'non-real gases' (as such category does not exist), but precisely to real gases.

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Most popular questions from this chapter

An ideal gas cannot be liquefied because (a) its critical temperature is always above \(0^{\circ} \mathrm{C}\) (b) its molecules are relatively smaller or in size (c) it solidifies before becoming a liquid (d) forces operative between its molecules are negligible

According to the van der Waals correction to get the pressure of ideal gas in observed pressure a definite fraction for correction is (a) subtracted (b) added (c) divided (d) unchanged

The gas which can be liquefied under high pressure and \(40^{\circ} \mathrm{C}\) is (a) nitrogen (b) hydrogen (c) oxygen (d) ammonia

Which one of the following gases has the maximum value of root mean square velocity? (a) \(\mathrm{CH}_{4}\) (b) \(\mathrm{CO}_{2}\) (c) \(\mathrm{H}_{2}\) (d) \(\mathrm{CO}\)

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 \(P\)
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