Which of the following is an assumption of the kinetic model of an ideal gas?
Correct answer: B. The collisions between particles are elastic
- A. The gas is at high pressure
- B. The collisions between particles are elastic
- C. There are weak forces of attraction between the particles in the gas
- D. The total energy of particles is proportional to the temperature
Explanation
OPTION A: The gas behave ideally at low pressure and at high temperature.OPTION B: According to KMT, all the collisions of a gas molecule are elastic, because the total energy of the molecule remains constant. Hence, B is the correct option.OPTION C: According to KMT, the attractive or repulsive forces among the gas molecules are negligible. Therefore, every gas molecule behaves independently.OPTION D: According to KMT, the average kinetic energy of gas molecules is directly proportional to absolute temperature.
Last updated
About Kinetic Molecular Theory
Kinetic molecular theory explains gases as rapidly moving particles separated by large distances, with negligible volume and negligible intermolecular attraction in the ideal model. It relates temperature to average kinetic energy and explains gas pressure, Boyle's and Charles's laws, diffusion, effusion and the conditions under which real gases deviate from ideal behavior.
Practise Gases
443 free Gases MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Exams that ask Chemistry questions like this
Chemistry is on 12 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
Related questions
A balloon filled with ethyne is pricked with a sharp pointed needle and quickly dropped in a tank of H2 gas under identical conditions. After a while the balloon will be:
A bottle of dry NH3 and a bottle of dry HCI connected through a long tube are opened simultaneously of both ends. The white NHCl ring formed will be
A fixed mass of an ideal gas is contained in a cylinder at a constant temperature. Now, the pressure of the gas is decreased. What happened to the molecules of gas?
A gas diffuses 1/2 times as fast as hydrogen, its molecular mass is:
A gas sample contains three molecules each having speeds 1 ms-1, 2 ms-1, and 3 ms-1. What is the mean square speed?