Kinetic Molecular Theory
Kinetic Molecular Theory attempts to explain why gas molecules behave as they do. It is based off four central tenets.
1. Gaseous molecules have no volume
2. Collisions between gaseous molecules are elastic (no energy is gained or lost)
3. Gaseous molecules have no attraction with one another
4. Average kinetic energy is related to the temperature of the molecules. KE=1.5RT (R = 8.3145J/(K x mol)
Relationships between Pressure, Volume, Moles, and Temperature
Pressure & Volume
P = (nRT)(1/V)
A decrease in volume results in more collisions by the particles with the walls of the container, increasing the pressure of the container.
Pressure and Temperature
An increase in temperature increases the kinetic energy of particles, resulting in the particles colliding with the walls of the container with greater force and frequency, thus increasing the pressure of the container.
P = (nR/V)T
Volume and Temperature
Increasing the temperature increases the force and frequency with which gas particles collide with the container of the walls. An increase in volume is needed in order to compensate and keep the pressure constant.
Volume and Number of Moles (Avogandro’s Law)
V = (RT/P)n
An increase in the number of moles of gas results in more collisions with the containers of the wall, thereby increasing the pressure. In order to compensate and keep the pressure constant, an increase in volume is needed, assuming the temperature is kept constant, in order to counter the increased gas particles.
P = (nRT)(1/V)
A decrease in volume results in more collisions by the particles with the walls of the container, increasing the pressure of the container.
Pressure and Temperature
An increase in temperature increases the kinetic energy of particles, resulting in the particles colliding with the walls of the container with greater force and frequency, thus increasing the pressure of the container.
P = (nR/V)T
Volume and Temperature
Increasing the temperature increases the force and frequency with which gas particles collide with the container of the walls. An increase in volume is needed in order to compensate and keep the pressure constant.
Volume and Number of Moles (Avogandro’s Law)
V = (RT/P)n
An increase in the number of moles of gas results in more collisions with the containers of the wall, thereby increasing the pressure. In order to compensate and keep the pressure constant, an increase in volume is needed, assuming the temperature is kept constant, in order to counter the increased gas particles.