(A) The average kinetic energy of an ideal gas is given by $K.E. = \frac{3}{2} nRT$ for $n$ moles of gas. For $1 \ mol$ of any ideal gas,$K.E. = \frac

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Kinetic energy of $1 \ mol$ of gas depends on mass of the gas molecule.

(A) The average kinetic energy of an ideal gas is given by $K.E. = \frac{3}{2} nRT$ for $n$ moles of gas. For $1 \ mol$ of any ideal gas,$K.E. = \frac{3}{2} RT$. This shows that the kinetic energy of $1 \ mol$ of an ideal gas depends only on the temperature $T$ and is independent of the nature of the gas (mass of the molecule). Therefore,the statement that kinetic energy depends on the mass of the gas molecule is false.

Class 11 Chemistry States of Matter Kinetic molecular theory of gases and Molecular collisions

Easy

Find the false statement for ideal gases.

AP EAMCET 2022 All AP EAMCET

A
Kinetic energy of $1 \ mol$ of gas depends on mass of the gas molecule.
B
Kinetic energy increases with increase in temperature.
C
Kinetic energy of $1 \ g$ of $H_2$ is higher than that of $8 \ g$ of $O_2$ at the same temperature.
D
At a given temperature,kinetic energy does not depend on the pressure of the gas.