The pressure exerted by the gas is directly proportional to the number of collisions per unit area.
Gases are all around us and affect our lives in various ways, from the atmosphere that envelops the Earth to the weather, to the changing colors of the sky in different times of the day, to daily life activities such as cooking, pumping tires, and filling up balloons for parties and celebrations.
The properties of gases can be explained in terms of the Kinetic Molecular Theory (KMT), proposed by two scientists, Ludwig Boltzman and James Maxwell, who were working separately in different countries, to explain the behavior of gases.
The Kinetic Molecular Theory of Gases (KMT) describes the behavior of gases in terms of particles in motion and makes several assumptions about the size, motion, and energy of gas molecules.
An increase in the temperature will increase the average kinetic energy of the gas particles causing the particles to move quickly, which allows the particles to collide more and thus increases the pressure.
The pressure of a gas increases as the temperature is increased and decreases as the temperature is lowered, entailing a linear dependency of pressure on temperature.
The volume of a gas increases as the temperature is increased and decreases as the temperature is lowered, entailing a linear dependency of volume on temperature.
The pressure of a gas is a result of the collisions between gas particles and with the walls of the container, according to the Kinetic Molecular Theory.
The volume of a gas increases as the temperature is increased and decreases as the temperature is lowered, implying a linear dependency of volume on temperature.
Based on the Kinetic Molecular Theory, when the pressure is constant, heating a gas will cause an increase in the average kinetic energy of gas particles.
The increase in the average kinetic energy of gas particles also increases the movement of each gas particle resulting to an increase in the number of collisions between the gas particles and with the wall of the container.
Changes in pressure won’t occur in Charles’ Law because the effect on pressure is being counteracted by an increase in the volume of the gas container.
Barometer, open-end manometers, and devices used in measuring the pressure of an atmospheric pressure enclosed gas are examples of devices used in measuring pressure.