Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 77

What are the basic assumptions of the kinetic molecular theory of gases? How does the kinetic molecular theory explain Boyle's law, Charles' law, Avogadro's law, and Dalton's law of partial pressures?

Short Answer

Expert verified
The basic assumptions of kinetic molecular theory are that gas molecules are in constant, random motion with no intermolecular forces. The theory explains Boyle's law, Charles' law, Avogadro's law, and Dalton's law by focusing on the behavior of gas molecules in relation to pressure, volume, temperature, and the number of molecules.

Step by step solution

01

Basic Assumptions of the Kinetic Molecular Theory

1. Gases consist of large number of molecules that are in constant, random motion. 2. The volume of the molecules in a gas is negligible compared to the volume of the gas itself. 3. The gas molecules are in perfectly elastic collision with each other and with the walls of their container. 4. There are no forces of attraction or repulsion between the molecules of a gas. 5. The average kinetic energy of gas molecules depends solely on the temperature of the gas.
02

Explanation of Boyle's law

According to Boyle's Law, the pressure of a gas is inversely proportional to its volume, assuming the temperature remains constant. Based on Kinetic Molecular Theory, as the volume decreases, the gas molecules have less space to move around and thus collide with the walls of the container more often, increasing pressure.
03

Explanation of Charles' law

Charles' law states that the volume of a gas is directly proportional to its absolute temperature, at constant pressure. From the kinetic molecular theory perspective, as the temperature increases, the kinetic energy of the gas molecules increases, causing them to move faster and collide with the walls of the container more forcefully and frequently, thus increasing the volume.
04

Explanation of Avogadro's law

Avogadro's law states that equal volumes of all gases at the same temperature and pressure contain the same number of molecules. This can be explained by the kinetic molecular theory as follows: the volume occupied by a gas is proportional to the number of gas molecules, regardless of the kind of gas.
05

Explanation of Dalton's law

Dalton's law of partial pressures states that the total pressure of a system is the sum of the partial pressures of its components. This is because, as per kinetic molecular theory, gas molecules are in constant, random motion and exert pressure independent of other gas molecules.

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

Which of the following has a greater mass: a sample of air of volume \(V\) at a certain temperature \(T\) and pressure \(P\) or a sample of air plus water vapor having the same volume and at the same temperature and pressure?

State Dalton's law of partial pressures and explain what mole fraction is. Does mole fraction have units?

Commercially, compressed oxygen is sold in metal cylinders. If a 120-L cylinder is filled with oxygen to a pressure of 132 atm at \(22^{\circ} \mathrm{C},\) what is the mass (in grams) of \(\mathrm{O}_{2}\) present? How many liters of \(\mathrm{O}_{2}\) gas at 1.00 atm and \(22^{\circ} \mathrm{C}\) could the cylinder produce? (Assume ideal behavior.)

The pressure of \(6.0 \mathrm{~L}\) of an ideal gas in a flexible container is decreased to one-third of its original pressure, and its absolute temperature is decreased by one-half. What is the final volume of the gas?

Consider this apparatus. When a small amount of water is introduced into the flask by squeezing the bulb of the medicine dropper, water is squirted upward out of the long glass tubing. Explain this observation. (Hint: Hydrogen chloride gas is soluble in water.)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

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