Question

1. according to the kinetic - theory of gases which of the following statements is correct

gas molecules collide with each other at high pressure only
at increased temperature gas molecules collide less often with the container walls
ideal gas molecules stick to each other at lower temperature
ideal gas molecules have finite mass but zero volume

Explanation:

Step1: Analyze gas - molecule collision

Gas molecules are in constant random motion and collide with each other and the container walls at all pressures, not just high - pressure. So the statement "Gas molecules collide with each other at high pressure only" is incorrect.

Step2: Examine effect of temperature on collisions

As the temperature of a gas increases, the average kinetic energy of the gas molecules increases. This means the molecules move faster and collide more frequently with the container walls. So the statement "At increased temperature gas molecules collide less often with the container walls" is incorrect.

Step3: Consider behavior of ideal gas molecules

Ideal gas molecules are assumed to have no intermolecular forces of attraction or repulsion, so they do not stick to each other at any temperature. So the statement "Ideal gas molecules stick to each other at lower temperature" is incorrect.

Step4: Recall properties of ideal gas molecules

One of the postulates of the kinetic theory of ideal gases is that ideal gas molecules have finite mass but zero volume. This is an idealized assumption that simplifies the mathematical treatment of gas behavior.

Answer:

Ideal gas molecules have finite mass but zero volume.