12th November 2019

britannica

14

What are the four basic assumptions of the kinetic theory?

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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

So, who proposed the kinetic molecular theory?

Unlike Lavoisier and Dalton, the 19th century German physicist Rudolf Clausius rejected caloric theory. Instead of regarding heat as a substance that surrounds molecules, Clausius proposed that heat is a form of energy that affects the temperature of matter by changing the motion of molecules in matter.

What are the main postulates of kinetic theory of gases?

9.12: Kinetic Theory of Gases: Postulates of the Kinetic Theory

1 The molecules in a gas are small and very far apart.
2 Gas molecules are in constant random motion.
3 Molecules can collide with each other and with the walls of the container.
4 When collisions occur, the molecules lose no kinetic energy; that is, the collisions are said to be perfectly elastic.

What are the four assumptions of the kinetic molecular theory?

GASES CONSIST OF LARGE NUMBERS OF PARTICLES THAT ARE FAR APART RELATIVE TO THEIR SIZE.
COLLISIONS BETWEEN GAS PARTICLES ARE ELASTIC COLLISIONS.
GAS PARTICLES ARE IN CONSTANT, RAPID, RANDOM MOTION.
THERE ARE NO FORCES OF ATTRACTION OR REPULSION BETWEEN GAS PARTICLES.

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What assumptions are made in the kinetic theory of ideal gases?

The ideal gas law can be derived from the kinetic theory of gases and relies on the assumptions that (1) the gas consists of a large number of molecules, which are in random motion and obey Newton's laws of motion; (2) the volume of the molecules is negligibly small compared to the volume occupied by the gas; and (3)

2

How is a real gas different from an ideal gas?

Real gases have small attractive and repulsive forces between particles and ideal gases do not. Real gas particles have a volume and ideal gas particles do not. Real gas particles collide in-elastically (loses energy with collisions) and ideal gas particles collide elastically.

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What are the three assumptions of the kinetic theory of gases?

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

4

What are the main postulates of kinetic theory of gases?

This theory is based on the following postulates, or assumptions. Gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion. Collisions between gas particles or collisions with the walls of the container are perfectly elastic.

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What is the kinetic theory in chemistry?

The kinetic theory describes a gas as a large number of submicroscopic particles (atoms or molecules), all of which are in constant rapid motion that has randomness arising from their many collisions with each other and with the walls of the container.

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Why is a gas easy to compress?

The atoms and molecules in gases are much more spread out than in solids or liquids. They vibrate and move freely at high speeds. A gas will fill any container, but if the container is not sealed, the gas will escape. Gas can be compressed much more easily than a liquid or solid.

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How does the kinetic theory explain the compressibility of gas?

The behavior of ideal gases is explained by the kinetic molecular theory of gases. Molecular motion, which leads to collisions between molecules and the container walls, explains pressure, and the large intermolecular distances in gases explain their high compressibility.

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What is the combined gas law used for?

The inter-dependence of these variables is shown in the combined gas law, which clearly states that: “ The ratio between the pressure-volume product and the temperature of a system remains constant.

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What is the kinetic molecular theory?

The Kinetic Molecular Theory. While the ideal gas law deals with macroscopic quantities of gas, the kinetic molecular theory shows how individual gas particles interact with one another. Gas molecules exert no force on each other unless they collide.

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What is the source of gas pressure?

The rapid motion and collisions of molecules with the walls of the container causes pressure (force on a unit area). Pressure is proportional to the number of molecular collisions and the force of the collisions in a particular area. The more collisions of gas molecules with the walls, the higher the pressure.

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What is the state of kinetic theory?

The Kinetic Theory of Matter states that matter is composed of a large number of small particles—individual atoms or molecules—that are in constant motion. This theory is also called the Kinetic-Molecular Theory of Matter and the Kinetic Theory of Gases.

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What is kinetic theory of gases in chemistry?

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.

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How does the kinetic theory of matter relate to solids liquids and gases?

The kinetic molecular theory of matter states that: Matter is made up of particles that are constantly moving. All particles have energy, but the energy varies depending on the temperature the sample of matter is in. This in turn determines whether the substance exists in the solid, liquid, or gaseous state.

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How do particles behave at the beginning at the boiling point and at the melting point?

Particles of a substance behave at its melting point by slipping out of the ordered arrangement of a solid due to energy that is required. 4Q. The particles of a substance behave at its boiling point by not being able to escape because of external pressure pushing down on the liquid.

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What are the three main factors that affect gas pressure?

Summary. An increase in the number of gas molecules in the same volume container increases pressure. A decrease in container volume increases gas pressure. An increase in temperature of a gas in a rigid container increases the pressure.

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What is an ideal gas in chemistry?

An ideal gas is a gas whose pressure P, volume V, and temperature T are related by the ideal gas law. PV = nRT, where n is the number of moles of the gas and R is the ideal gas constant. Ideal gases are defined as having molecules with negligible size with an average molar kinetic energy dependent only on temperature.

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What causes gas pressure using the kinetic theory?

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 hits the wall, it exerts a force on the wall.

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What are the properties of a gas?

Gases have three characteristic properties: (1) they are easy to compress, (2) they expand to fill their containers, and (3) they occupy far more space than the liquids or solids from which they form. An internal combustion engine provides a good example of the ease with which gases can be compressed.

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How do particles move in a gas?

gas vibrate and move freely at high speeds. liquid vibrate, move about, and slide past each other. solid vibrate (jiggle) but generally do not move from place to place.

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What are three assumptions about particles in a gas are made by the kinetic energy?

According to kinetic theory: Gases consist of particles in constant, random motion. They continue in a straight line until they collide with something—usually each other or the walls of their container. Particles are point masses with no volume.

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