There are no attractive forces between the molecules of gas.

The average kinetic energy of the particles in a gas is proportional to the temperature of the gas. If they move faster, the particles will exert a greater force on the container each time they hit the walls, which leads to an increase in the pressure of the gas.

The pressure of a gas is a measure of the linear momentum of the molecules. As the gas molecules collide with the walls of a container, the molecules impart momentum to the walls, producing a force that can be measured. The force divided by the area is defined to be the pressure.

The kinetic molecular theory (KMT) describes the behavior of ideal gases at the particle level.

the basics of the Kinetic Molecular Theory of Gases (KMT) should be understood. This model is used to describe the behavior of gases. More specifically, it is used to explain macroscopic properties of a gas, such as pressure and temperature, in terms of its microscopic components, such as atoms.

In gases the particles move rapidly in all directions, frequently colliding with each other and the side of the container. With an increase in temperature, the particles gain kinetic energy and move faster.

The three main principles of the kinetic theory are:

• No energy is gained or lost during the collision between molecules.
• Molecules take up a negligible amount of space in relation to the container space they occupy.
• The molecules are in constant linear motion.

Kinetic theory explains macroscopic properties of gases, such as pressure, temperature, viscosity, thermal conductivity, and volume, by considering their molecular composition and motion. individual gas particles collide with the walls of the container thus producing a force.

KE=31​mnv−2. where, n is the number of molecules and v− is the average speed of molecules.

The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the …

The kinetic-molecular theory of gases assumes that ideal gas molecules (1) are constantly moving; (2) have negligible volume; (3) have negligible intermolecular forces; (4) undergo perfectly elastic collisions; and (5) have an average kinetic energy proportional to the ideal gas’s absolute temperature.

KMT links the microscopic behaviors of ideal gas molecules to the macroscopic properties of gases. In its current form, KMT makes five assumptions about ideal gas molecules: Gases consist of many molecules in constant, random, linear motion. The volume of all the molecules is negligible compared to the gas’s total volume.

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By making several assumptions about the motion and energy of molecules, KMT provides scientists with a useful framework for understanding how the behavior of molecules influences the behaviors of different states of matter, particularly the gas state.

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