Question

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 1

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.

Answer 2

Concerning ideal gases, the gases exert pressure as a result of the collisions of the gas molecules with the walls of the container. Hence, option (C) is correct.

What is an Ideal Gas?

The gas particles which are known for their ideal behavior like no interaction with other particles, take up no space (have no volume), are known as an ideal gas. These kinds of gases are only reference gases.

Now as per the given problem,

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

• Statement B  is incorrect because, at STP, an equal volume of all gases has the same number of molecules.

• Statement D  is incorrect because the ideal gas works well when the intermolecular force of attraction between the gas molecules is negligible.

• Statement C  is correct because when molecules collide with the wall of the 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 the more the particles hit the walls of a container, the higher the pressure.

Thus, we can conclude that concerning ideal gases, the gases exert pressure as a result of the collisions of the gas molecules with the walls of the container.

Learn more about the ideal gases here:

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