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(A) The average molar kinetic energy of an ideal gas is given by the expression $\overline{K.E.} = \frac{3}{2}RT$. Since the average molar kinetic ene

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$\overline{KE}_{CO} = \overline{KE}_{N_2}$

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(A) The average molar kinetic energy of an ideal gas is given by the expression $\overline{K.E.} = \frac{3}{2}RT$. Since the average molar kinetic energy depends only on the temperature $(T)$ and the universal gas constant $(R)$,it is independent of the nature of the gas or its molecular mass. Therefore,at the same temperature,the average molar kinetic energy of $CO$ and $N_2$ molecules will be equal. Thus,$\overline{KE}_{CO} = \overline{KE}_{N_2}$.

Which of the following expressions correctly represents the relationship between the average molar kinetic energy,$\overline{K.E.}$,of $CO$ and $N_2$ molecules at the same temperature?

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