Which of the following expressions correctly represents the relationship between the average molar kinetic energies `(KE)` of `CO` and `N_(2)` molecules at the same temperature?

On the basis of the postulates of kinetic theory of gases, it is possible to derive the mathematical expression, commonly known as kinetic gas equation. PV = 1/3 m n u^3? where, P= Pressure of the gas, V a volume of the gas, m=Mass of a molecule, n = Number of molecules present in the given amount of a gas and u = root mean square speed For one mole of gas, PV = RT and n=N_A 1/3 m N_a u^2 = RT or 2/3 .1/2m N_A u^2 = N_A [1/2mN_Au^2 = KE "per mole"] ,2/3K.E. = RT implies K.E. 3/2RT Average kinetic energy per mol does not depend on the nature of the gas but depends only on temperature. This, when two gases are mixed at the same temperature, there will be no rise or decrease in temperature unless both react chemically. Average kinetic energy per molecule = ("Average K.E. per mole")/N = 3/2(RT)/(N) implies 3/2kT where k is the Boltzmann constant Which of the following expressions correctly represents the relationship between the average molar kinetic energies of CO and N_2 molecules at the same temperature ?

Which of the following expressions correctly represents the relationship between the average molar kinetic energy bar(KE) of CO and N_(2) molecules at the same temperature ?

Which of the following expressions CORRECTLY represents the relationship between the average molar kinetic energy, K.E. of CO and N_(2) molecules at the same temperature?

Which of the following diagrams correctly represents the relationship between automobile cars and motorcycles?

Which of the following relations represents the relationship between the average speed, time and distance correctly?