Which of the following is NOT a true statement of the kinetic Theory of Gases?

Sammyporsche123

2 years ago

The statement that is NOT true according to the kinetic theory of gases is **D. Every molecule has the same kinetic energy at a particular temperature**.

In a gas, individual molecules do not all have the same kinetic energy at a given temperature. Instead, they have a range of kinetic energies that is described by the Maxwell-Boltzmann distribution. While the average kinetic energy of the molecules is proportional to the absolute temperature of the gas (statement E), individual molecules can have kinetic energies that are higher or lower than this average.

Therefore, all other options (A, B, C, and E) are correct statements according to the kinetic theory of gases. So, the correct answer is **D**.

Som15432

1 year ago

Let's break down each statement to find the one that's NOT true:
* A. The molecules move at random: This is true! Gas molecules are constantly moving in all directions.
* B. The size of molecules is negligible as compared with the volume of gas: Also true! Gas molecules are tiny compared to the space they occupy.
* C. The molecular collisions are perfectly elastic: This is also true! In a perfectly elastic collision, no kinetic energy is lost.
* D. Every molecule has the same kinetic energy at a particular temperature: This is NOT true! While the average kinetic energy is the same at a given temperature, individual molecules move at different speeds, so they have different kinetic energies.
* E. The average kinetic energy is proportional to the absolute temperature of the gas: This is true! As temperature increases, the average speed of the molecules increases, and so does their average kinetic energy.
So, the answer is D. Every molecule has the same kinetic energy at a particular temperature.