How does kinetic theory explain gas pressure?

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Oscar Sauer asked a question: How does kinetic theory explain gas pressure?
Asked By: Oscar Sauer
Date created: Tue, Apr 6, 2021 10:41 AM
Date updated: Wed, Nov 23, 2022 1:44 AM

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Video answer: Kinetic theory of gases: pressure derivation

Kinetic theory of gases: pressure derivation

Top best answers to the question «How does kinetic theory explain gas pressure»

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.

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The kinetic molecular theory can be used to explain each of the experimentally determined gas laws. The pressure of a gas results from collisions between the gas particles and the walls of the container. Each time a gas particle

How does the kinetic molecular theory of gases explain gas pressure? The concept of pressure is explained in kinetic theory as a consequence of kinetic energy of gases. Due to the troublesome motion of the gas molecules, they will collide with each other, some of them shall collide with the container walls and then bounce back and this process continues.

The pressure of a gas results from collisions between the gas particles and the walls of the container. Each time a gas particle hits the wall, it exerts a force on the wall. Considering that fact, how does the kinetic molecular theory

Correct answer to the question How does kinetic theory explain gas pressure - hmwhelper.com What is the main reason why some developing countries fear the increase the free trade policies around the world?

Kinetic Molecular Theory states that gas particles are in constant motion and exhibit perfectly elastic collisions. Kinetic Molecular Theory can be used to explain both Charles’ and Boyle’s Laws. The average kinetic energy of a collection of gas particles is directly proportional to absolute temperature only.

In the kinetic theory of gases, the pressure is assumed to be equal to the force (per unit area) exerted by the atoms hitting and rebounding from the gas container's surface. Consider a gas of a large number N of molecules, each of mass m, enclosed in a cube of volume V = L3.

When a gas is heated, its temperature increase. Explain it on the basis of kinetic theory of gases. asked Jan 30 in Physics by Raadhi (34.5k points) kinetic theory class-11 0 votes 1 answer Derive Dalton’s law of practical asked ...

In the kinetic theory of gases, gas molecules move around in the most random way colliding and bumping into each other and then bouncing off in the opposite direction. The molecules exert no intermolecular forces on each other and they have no potential energy associated with them in their motion. Thus the energy is wholly kinetic. The concept of pressure is explained in kinetic theory as a ...

The kinetic molecular theory explains the pressure exerted by gases as the result of many collissions of the gas particles (atoms or molecules) with the walls of the vessel where they are contained. The pressure is the perpendicular force per unit area exerted by the gas particles when they hit the walls of the container.

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Video answer: Kinetic molecular theory and its postulates

Kinetic molecular theory and its postulates