kinetic molecular theory of gases

• 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.
• The Kinetic Molecular Theory explains why gases behave as they are.
• A gas is composed of a very large number of extremely small particles (molecules or, in some cases, atoms) in constant, random, straight-line motion.
• Molecules of a gas are separated by great distances, making the gas mostly empty space.
• 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 relationship among pressure, temperature, and volume of a fixed amount of gas is described by Boyle's Law, Charles's Law, and Avogadro's Law.
• 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 three variables in Boyle's Law, Charles's Law, and Avogadro's Law have the same relationships as those in the three preceding gas laws.
• At constant volume, the pressure of a gas is proportional to the number of moles of the gas, according to Avogadro's Law.
• In Gay-Lussac’s Law, the volume is held constant, and the change in temperature greatly affects the pressure of the gas.
• 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.
• Doubling the temperature of a gas likewise doubled the pressure.
• When the Kelvin temperature is reduced by one-half, the volume also decreases by one-half.
• The volume of a gas molecule is very small and negligible compared to the volume of its gas.
• The interaction among particles, either attractive and repulsive forces between the molecules, are negligible.
• The increase in the volume of the gas will increase the distance between gas particles and so decreases the collisions.
• 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.
• When volume is plotted against 1/P, the graph is a straight line.
• At constant P and n, V ∝ T and V = constant.
• Doubling the Kelvin temperature of a gas causes the volume to double.
• When the Kelvin temperature is reduced by one-half, the volume also decreases by one-half.
• 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.
• The increase in the number of collisions will supposedly lead to an increase in gas pressure.
• Amonton’s Law states that at constant volume, the pressure of a fixed amount of gas is directly proportional to its temperature.
• 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.
• The temperature to be used in the calculations must be absolute (in K), T = 273 + ℃.
• The Combined Gas Law is a combination of Boyle’s, Charles’, and Amonton’s Laws.
• The volume of a gas is equal to the size of the container in which the gas is placed.
• The temperature of gases is expressed in terms of Kelvin temperature.
• 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.
• Boyle’s Law states that at constant temperature, the volume of a fixed quantity of gas is inversely proportional to the pressure.
• At Standard Condition (STP), temperature is 273.15 K, pressure is 1 atm, and volume is 22.4 L.
• The standard temperature is 273.15 K.
• The quantity of gas present in a container is referred to as the amount of gas (n).
• Unit for the amount of gas (n) is in grams and moles.