Science kinetic molecular theory

• The Kinetic Molecular Theory (KMT) helps us to explain why matter exists in different phases (i.e. solid, liquid, and gas), and how matter can change from one phase to the next.
• t says that all matter is composed of particles that have a certain amount of energy which allows them to move at different speeds depending on the temperature (energy).
• There are spaces between the particles and attractive forces between particles when they come close together
• The average speed of particles increases as temperature increases.
• The Kinetic Molecular Theory of Gases explains the properties of gases and describes the behavior of gases.
• The distances from one molecule to another molecule are far greater than the molecules’ dimensions
• molecules can be considered as spherical bodies which possess negligible mass and volume.
• Gases are composed of molecules
• Gas molecules are always in constant random motion, and they frequently collide with one another and with the walls of the container.
• Collision among molecules is perfectly elastic
• energy may transfer from molecule to molecule as the result of the collision but the total energy of all the molecules in the system remain the same/constant.
• There is neither attractive nor repulsive force between or among gas molecules.
• Movement of gas molecules is affected by temperature.
• The average kinetic of the molecules is directly related to the temperature of the gas.
• In the KMT, pressure is the force exerted against the wall of a container by the continual collision of molecules against it.
• The pressure of a gas results from collisions between the gas particles and the walls of the container.
• An increase in the number of gas particles in the container increases the frequency of collisions with the walls and therefore the pressure of the gas increases
• The last postulate of the kinetic molecular theory states that the average kinetic energy of a gas particle depends only on the temperature of the gas.
• the average kinetic energy of the gas particles increases as the gas becomes warmer.
• the mass of these particles is constant, the kinetic energy can only increase if the average velocity of the particles increased.
• Since the force per collision becomes greater as the temperature increases, the pressure of the gas must increase as well.
• When a gas is compressed without changing its temperature, the average kinetic energy of the gas particles stays the same
• The volume of a gas is directly related to its temperature at constant pressure.
• The pressure of a gas is directly related to its temperature at a constant temperature
• o The volume of a gas is inversely related to its pressure at a constant temperature
• The increase of the number of gas particles, the pressure of gas increases.