At low temperatures it is assumed that the volume of a gas(an ideal gas) is zero
and also they show no attraction or repulsion. it is incorrect.
Real gases have non-zero volume and experience intermolecular forces, which contradict the assumptions of kinetic-molecular theory that gases consist of point particles with no volume and that there are no intermolecular forces present. Real gases also deviate from ideal behavior at high pressures and low temperatures, which is not accounted for in the kinetic-molecular theory.
An ideal gas. Ideal gases are theoretical gases that perfectly follow the assumptions of the kinetic molecular theory and gas laws, such as having particles that are point masses and exhibit perfectly elastic collisions.
kinetic theory.
The process of gas molecules in a container moving in straight lines, colliding with each other and the walls of the container can be explained by the kinetic-molecular theory. This theory describes how the behavior of gas molecules is influenced by their motion and energy.
temperature in kelvin
Real gases have non-zero volume and experience intermolecular forces, which contradict the assumptions of kinetic-molecular theory that gases consist of point particles with no volume and that there are no intermolecular forces present. Real gases also deviate from ideal behavior at high pressures and low temperatures, which is not accounted for in the kinetic-molecular theory.
Rapid Motion does.
Kinetic Molecular Theory's abbreviation is KMT or sometimes KMTG when it is the abbreviation for Kinetic Molecular Theory of Gas
The Kinetic Molecular Theory does not have a specific formula. It is a set of assumptions that describe the behavior of gases based on the motion of their particles. These assumptions include that gases are composed of particles in constant random motion, have negligible volume, and do not exert intermolecular forces except when they collide.
The kinetic-molecular theory does not work well at describing the behavior of particles under conditions of high pressure or low temperature, where intermolecular forces become significant. Additionally, it may not accurately predict the behavior of real gases due to assumptions such as negligible volume of particles and no intermolecular forces between them.
Diffusion can be explained by the kinetic-molecular theory.
I researched and all I found for The Kinetic-Molecular Theory was this:KE = 1/2 mv2
An ideal gas. Ideal gases are theoretical gases that perfectly follow the assumptions of the kinetic molecular theory and gas laws, such as having particles that are point masses and exhibit perfectly elastic collisions.
At high pressure, the assumptions of kinetic molecular theory may no longer hold true as the molecules are squeezed close together and their interactions become significant. This can lead to deviations from the ideal gas behavior predicted by the theory, such as changes in volume and temperature. These deviations are more pronounced for real gases than ideal gases under high pressure conditions.
kinetic theory.
The father of the Kinetic Molecular Theory of Gases is James Clerk Maxwell. He made significant contributions to the theory by formulating the concept of the distribution of molecular speeds in a gas.
because kinetic energy have electltrolises