Kinetic Theory of Gases 2023 with 100% correct questions and answers

Gases are mostly empty space the total volume of the molecules is negligibly small compared with that of the container to which they are confined Gas molecules are in constant, chaotic motion They collide frequently with one another and with the container walls. Their velocities are constantly changing Collisions are elastic There are no attractive forces that would tend to make molecules stick to one another or to the container walls. Gas pressure is caused by the collision of molecules with the walls of the container Pressure increase with energy and frequency of collisions Pressure The more molecules there are in a given volume, the greater the collision frequency and so the greater the pressure. Pressure is directly related to energy of collision (mass x u^2) Average Kinetic Energy Equation contains three constants (3/2, R, NA) and only one variable, the temperature T. Average Kinetic Energy of Translational Motion At a given temperature, molecules of different gases must all have the same average kinetic energy of translational motion. Average kinetic energy of a gas molecule is directly proportional to the temperature in Kelvins Average speed speed depends on both temperature and molar mass. Average speed is directly proportional to the square root of the absolute temperature, and inversely proportional to the square root of molar mass (MM). For two different gases A and B at the same temperature. Effusion of Gases depends on pressures of gases and the relative speed of their particles. At constant pressure, and temperature, the rate of effusion = square root of molar mass. At a given temperature and pressure, the rate of effusion of a gas, in moles, per unit time, is inversely proportional to the square root of its molar mass. Density of Gas decrease in pressure = increase in density increase in temperature = decrease in density molar mass is directly proportional to molar mass