Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 18: Problem 14

In what sense can a gas of diatomic molecules be considered an ideal gas, given that its molecules aren't point particles?

Short Answer

Expert verified
A gas of diatomic molecules can be considered an ideal gas because, even though its molecules are not point particles, under most conditions the volume of the individual molecules is negligible compared to the overall volume of the gas. The significant intermolecular distances make it possible to treat them as point particles, conforming to the properties of an ideal gas.

Step by step solution

01

Define the Ideal Gas

An ideal gas is a theoretical gas composed of a set of randomly-moving, non-interacting point particles. The ideal gas concept is used because it simplifies the mathematical equations used to describe the behavior of gases. Real gases obey these ideal behaviors to a good approximation only under high temperature and low pressure conditions. The randomness ensures that the gas’s overall behavior can be described using statistical methods.
02

Understanding Point Particles

In physics, a point particle is an idealized object which is treated as being dimensionless ‑ in the sense it has no spatial extent, which simplifies many physics problems. In the context of a gas, point particles mean that the individual particles of the gas do not occupy physical volume. The ideal gas law's validity assumes that the molecules of the gas are point particles, resulting in minimal intermolecular forces.
03

Relating Diatomic Gas Molecules to Ideal Gas

A diatomic molecule consists of two atoms bonded together. Even though they aren't point particles, under most conditions, we can still treat them as such. The volumes of the gas molecules themselves are tiny compared to the total volume of the gas. Hence, they can be considered as point particles in this context. Specifically, in many cases, the size of diatomic molecules is much smaller than the average distance between them, especially under typical pressure and temperature conditions. That’s why, although diatomic gases exactly aren't point particles, they can still be approximated as ideal gases.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A gas expands isothermally from state \(A\) to state \(B,\) in the process absorbing 35 J of heat. It's then compressed isobarically to state \(C,\) where its volume equals that of state \(A .\) During thecompression, \(22 \mathrm{J}\) of work are done on the gas. The gas is then heated at constant volume until it returns to state \(A\). (a) Draw a \(p V\) diagram for this process. (b) How much work is done on or by the gas during the complete cycle? (c) How much heat is transferred to or from the gas as it goes from \(B\) to \(C\) to \(A\) ?

Are the initial and final equilibrium states of an irreversible process describable by points in a \(p V\) diagram? Explain.

A gas with \(\gamma=1.40\) is at 100 kPa pressure and occupies \(5.00 \mathrm{L}\) (a) How much work does it take to compress the gas adiabatically to \(2.50 \mathrm{L} ?\) (b) What's its final pressure?

Your class on alternative habitats is designing an underwater habitat. A small diving bell will be lowered to the habitat. A hatch at the bottom of the bell is open, so water can enter to compress the air and thus keep the air pressure inside equal to the pressure of the surrounding water. The bell is lowered slowly enough that the inside air remains at the same temperature as the water. But the water temperature increases with depth in such a way that the air pressure and volume are related by \(p=p_{0} \sqrt{V_{0} / V},\) where \(V_{0}=17 \mathrm{m}^{3}\) and \(p_{0}=1\) atm are the surface values. Suppose the diving bell's air volume cannot be less than \(8.7 \mathrm{m}^{3}\) and the pressure must not exceed 1.5 atm when submerged. Are these criteria met?

Some water is tightly sealed in a perfectly insulated container. Is it possible to change the water temperature? Explain.
See all solutions

Recommended explanations on Physics Textbooks

Turning Points in Physics

Read Explanation

Circular Motion and Gravitation

Read Explanation

Medical Physics

Read Explanation

Scientific Method Physics

Read Explanation

Particle Model of Matter

Read Explanation

Nuclear Physics

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free