Individual collisions can transfer energy either way, depending on whether the gas X or Y molecule has greater energy. The collisions will sometimes transfer energy from a gas X molecule to a gas Y molecule and sometimes from Y to X. The final distribution of molecular speeds will result in a temperature between the two initial temperatures, at a value that depends on the relative numbers of the two types of molecules. Gas X has more molecules, so the final temperature will be closer to the initial temperature of gas X.

The average kinetic energy of gas molecules increases with increasing temperature.The average speed of gas molecules decreases with decreasing temperature.The temperature of a gas sample is independent of the average kinetic energy.There are gas molecules that move faster than the average.All the gas molecules in a sample cannot have the same kinetic energy.

As the temperature of a chemical reaction increases, the rate of reaction increases becauseA fewer particle collisions occurB the required activation energy increasesC more effective particle collisions occurD the concentration of the reactants increases

Temperature as the average kinetic energy of a gas increases.

At ordinary temperatures, the molecules of an ideal gas have only translational and rotational kinetic energies. At higher temperatures, they may also have vibrational energy. As a result, at higher temperatures

which parameter is same for molecules of all gases for given temperature