# 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.
A.

### 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.
• #### Who came up with the kinetic theory of gases?

In 1859, after reading a paper on the diffusion of molecules by Rudolf Clausius, Scottish physicist James Clerk Maxwell formulated the Maxwell distribution of molecular velocities, which gave the proportion of molecules having a certain velocity in a specific range. This was the first-ever statistical law in physics.
• #### What is the molecular kinetic theory of matter?

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.
• #### 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.
B.

### What are the four basic assumptions of the kinetic theory?

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
• #### 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.
• #### 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.
• #### 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.
C.

### 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 measurable characteristics of a gas?

Measurable Properties of Gases
• (1) The characteristics of gases are described fully in terms of four parameters or measurable properties:
• (i) The volume, V, of the gas.
• (ii) Its pressure, P.
• (iii) Its temperature, T.
• (iv) The amount of the gas (i.e., mass or number of moles).
• #### What are the 4 components of the kinetic molecular theory?

There are three main components to kinetic theory:
• No energy is gained or lost when molecules collide.
• The molecules in a gas take up a negligible (able to be ignored) amount of space in relation to the container they occupy.
• The molecules are in constant, linear motion.
• #### What are the basic assumptions of 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

Updated: 12th November 2019