When gas molecules collide with the walls of the container, the collision is elastic. ie. Momentum before collision = Momentum after collision. Hence, the gas molecule imparts a certain momentum to the wall. As there are a large no of gas molecules, a large no of molecules collide with the wall every second. Change in momentum per unit time (per second) is force. Force per unit area is pressure. This is the pressure exerted by gas molecules.
yes.. when applied with Boyle's law and Charles law and Gay Lussac's law, It can explain the pressure exerted by the gases
Consider a container full of gas particles. The gaseous particles move around with kinetic energy, therefore a velocity and momentum.
When these particles collide with the walls of the containers, they will 'bounce off'. This change in velocity, or change in momentum, ΔP, will be due to a force, F, which is in effect for the time it takes for the particle to 'bounce off' the container walls, Δt. Where F = ΔP/Δt.
Each molecule will exert this force on the container wall. The number of particles colliding with the container walls over a certain area will depend on the number of gas particles within the container. The combined force, F, of the gas particles which hit an area, A, of the container wall will create a pressure, p. Where p = F/A.
You see, when you fart, it is gas pressure being let out through your anus. :)
yes.. when applied with Boyle's law and Charles law and Gay Lussac's law, It can explain the pressure exerted by the gases
Gas pressure is caused by collisions between the representative particles of the gas and the inside walls of the container that they're in.
kinetic theory of gas is defined with the help of maxwell distribution
In an ideal gas, molecules don't take up space, and don't have long-range interactions.
temperature in kelvin
an ideal gas
Kinetic Molecular Theory of Gases
Kinetic theory explains the measurable volume of a gas, by stating that, the volume of a gas is inversely proportional to the pressure exerted on it, where pressure is created by the number of molecular collisions.
When it conforms to all assumptions of kinetic theory
Kinetic Molecular Theory's abbreviation is KMT or sometimes KMTG when it is the abbreviation for Kinetic Molecular Theory of Gas
interpretation of pressure on kinetic theory of gases
kinetic theory of gas is defined with the help of maxwell distribution
In an ideal gas, molecules don't take up space, and don't have long-range interactions.
According to the kinetic theory, the particles in a gas are considered to be small, hard spheres with an insignificant volume, and all the collisions between particles in a gas are perfectly elastic.
By looking at the states of matter ( solid ,liquid or gas) we can determine that a giben sample will have how much energy. Molecules in solid have least kinetic energy. Molecules in vapor (gas) have highest kinetic energy. Liquids have moderatee kinetic energy.
It is called compressibility. The compressibility of gases can be explained by the kinetic particle theory: due to the large amount of space between the gas particles and the weak attraction forces between them, gases can easily be compressed (the particles are brought closer to each other, thus reducing the volume of the gas).
The kinetic energy of a single gas molecule is not proportional to anything. The average kinetic energy of gas molecules is proportional to their absolute temperature.
The kinetic energy of a single gas molecule is not proportional to anything. The average kinetic energy of gas molecules is proportional to their absolute temperature.
The kinetic molecular theory assumes that the collisions of gas particles are perfectly elastic. This means that