Deviations from the ideal gas law are observed at high pressure and low temperature. Explain thi

Deviations from the ideal gas law are observed at high...

Key Concepts

Kinetic Molecular Theory

Kinetic molecular theory explains the macroscopic properties of gases by considering them as a large number of small particles moving in constant motion. It makes foundational assumptions such as perfectly elastic collisions, random motion, and negligible intermolecular forces and molecular volumes, which underlie the derivation of the ideal gas law.

Ideal Gas Law Assumptions

The ideal gas law is derived under the assumption that the gas molecules have no volume and do not interact with each other, except during elastic collisions. At high pressures and low temperatures, these assumptions break down because molecular distances decrease, making the finite size of molecules and the forces between them significant, thus leading to deviations from ideal behavior.

Intermolecular Forces

Intermolecular forces refer to the attractive or repulsive forces that occur between molecules. In the context of real gases, especially at low temperatures, these forces can reduce the kinetic energy of the molecules by causing attractions, which affects the pressure exerted by the gas and leads to deviations from the expected behavior predicted by the ideal gas law.

Finite Molecular Volume

The concept of finite molecular volume acknowledges that gas molecules occupy space. Under high-pressure conditions, the volume occupied by the gas molecules themselves becomes a significant fraction of the total volume, reducing the space available for molecular motion and leading to deviations from the ideal gas law predictions.

Transcript

00:01 Question number 24.

00:04 Division from id gas, from id gas are observed at high pressure and low temperature.

00:26 We want to explain this in the light of kinetic molecular theory.

00:31 Kinetic molecular theory explanation.

00:47 So to explain the note that at high pressure, the finite volume of gas particle finite volume of gas particle becomes appreciable appraisable we should know that i think gas law assume that the volume of particle of gas are negligible let me draw two bucks and i draw another one of the same so if this container has like a kind of covering.

02:12 So i have this volume, very large volume and this i have one particle.

02:20 This is a particle and i have this particle, the same particle here.

02:30 Just one.

02:32 Or maybe i have like one particle or two particles.

02:35 I can't let me just have like two.

02:38 I have two particle.

02:47 So the volume of this container, if the volume of this container is like let's say it's 1 ,000 later i'm just assuming this container is so bleak but the volume of this of each of the particle is just like maybe 0 .1, 1 .0 .00, there's a 001 later and i have two of it.

03:19 The volume of both of them will be 0 .002 later.

03:26 So the volume of the particle, this particle is negligible.

03:32 It's not appreciable when we compare to the total volume...

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