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Kinetic Molecular

Kinetic Molecular Theory

TermDefinition
Kinetic-Molecular Theory Theory based on the idea that particles of matter are always in motion.
First Assumption Gases consist of large numbers of tiny particles that are far apart relative to their size. The volume of gas particles are considered to be negligible (or zero).
Second Assumption Collisions (between gas particles and container walls and , between particles) are elastic collisions (kinetic energy (or KE) is conserved). Pressure exerted by gases is caused by collisions of the gas molecules within the walls of the container.
Third Assumption Gas particles are in continuous, rapid, random motion and possess KE.
Fourth Assumption There are no forces of attraction or repulsion between gas particles.
Fifth Assumption The average KE of gas particles depends on the temp. of the gas; KE=1/2mv^2 a. Mass is a constant. b. KE is dependent upon velocity (v) or speed (speed increases with an increase in temp.). c. Gases at the same temp. have the same average KE.
Kinetic Energy The energy of motion.
Ideal Gas A hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory.
Elastic Collision Collision in which there is no net loss of total kinetic energy.
Diffusion (Assumption 3) Spontaneous mixing of the particles of two substances caused by their random motion.
Effusion (Assumption 3) A process by which gas particles pass through a tiny opening.
Real Gas A gas that does not behave completely according to the assumptions of the kinetic-molecular theory.
Expansion (Assumption 3 & 4) Gases spontaneously fill the container they occupy.
Fluidity (Assumption 4) Gas particles glide past one another.
Low Density (Assumption 1) The gaseous state is 1/1000 the density of the liquid state.
Compressibility (Assumption 1) The volume of a gas can be decreased.
How Real Gases differentiate from Ideal Gases 1. High Pressure: the vol. of particles can no longer be considered zero. 2. Low Temp.: KE is no longer high enough to overcome attractive forces. 3. Polar Gases: The more polar the gas is, the greater the attractive force (because of partial charges).
Created by: syd._.waldron
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