Which of the following statements is true concerning ideal gases? A. The temperature of the gas sample is directly related to the average velocity of the gas particles. B. At STP, 1.0 L of Ar (g) contains about twice the number of atoms as 1.0 L of Ne (g) since the molar mass of Ar is about twice that of Ne. C. A gas exerts pressure as a result of the collisions of the gas molecules with the walls of the container. D. The gas particles in a sample exert attraction for one another. E. All of the above are false

Answer : The correct statement is (C).

Explanation:

Statement A : This statement is incorrect because the temperature of the gas sample is directly related to the average kinetic energy of the gas particles.

Statement B : This statement is incorrect because at STP, equal volume of all gases have the same number of molecules.

Statement D : This statement is incorrect because the ideal gas works well when the inter-molecular force of attraction between the gas molecules are negligible.

Statement C : This statement is correct because when molecules collides with the wall of container, they exert small force on the wall of the container. The pressure exerted by the gas is due to the sum of all the collision forces. That means more the particles hit the walls of container, the higher the pressure.