Question

xvii)
According to the kinetic theory of gases the absolute temperature of a perfect gas is
* Inversely proportional to the K.E of the molecules
* Independent of the K.E of the molecules
* Directly proportional to average translational K.E of the molecules
Equal to the K.E of the molecules

Answer 1

Answer:

all the gaseous particles are in in constant random motion at temperature above absolute zero

Answer 2

Answer:

Kinetic Molecular Theory of Gases

Jessie A. Key and David W. Ball

Learning Objectives

State the major concepts behind the kinetic molecular theory of gases.

Demonstrate the relationship between kinetic energy and molecular speed.

Apply the kinetic molecular theory to explain and predict the gas laws.

Gases were among the first substances studied using the modern scientific method, which was developed in the 1600s. It did not take long to recognize that gases all shared certain physical behaviours, suggesting that gases could be described by one all-encompassing theory. The

kinetic molecular theory of gases

is a model that helps us understand the physical properties of gases at the molecular level. It is based on the following concepts:

Gases consist of particles (molecules or atoms) that are in constant random motion.

Gas particles are constantly colliding with each other and the walls of their container. These collisions are elastic; that is, there is no net loss of energy from the collisions.

Gas particles are small and the total volume occupied by gas molecules is negligible relative to the total volume of their container.

There are no interactive forces (i.e., attraction or repulsion) between the particles of a gas.

The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and all gases at the same temperature have the same average kinetic energy.

Figure 6.6 “The Kinetic Molecular Theory of Gases” shows a representation of how we mentally picture the gas phase.

Figure 6-6

The kinetic molecular theory of gases describes this state of matter as composed of tiny particles in constant motion with a lot of distance between the particles. Because most of the volume occupied by a gas is empty space, a gas has a low density and can expand or contract under the appropriate influence. The fact that gas particles are in constant motion means that two or more gases will always mix as the particles from the individual gases move and collide with each other. The number of collisions the gas particles make with the walls of their container and the force with which they collide determine the magnitude of the gas pressure.

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