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Average molar kinetic energy of CO and $N_2$ at same temperature is :
A
$KE_1 = KE_2$
B
$KE_1 \gt KE_2$
C
$KE_1 \lt KE_2$
D
Can't say anything. Both volumes are not given
Detailed Solution
According to the kinetic theory, the average kinetic energy of gas molecules depends only on the absolute temperature: $KE = \dfrac{3}{2}RT$ per mole (translational).
It does not depend on the nature, mass or volume of the gas.
So at the same temperature, CO and $N_2$ have the same average molar kinetic energy: $KE_1 = KE_2$. (They even have the same molar mass, 28 g/mol.)
It does not depend on the nature, mass or volume of the gas.
So at the same temperature, CO and $N_2$ have the same average molar kinetic energy: $KE_1 = KE_2$. (They even have the same molar mass, 28 g/mol.)