Answer:
The false statement is C).
Explanation:
Individual molecules of an ideal gas could have any velocity, and so, any kinect energy. Temperature is related to the average kinectic energy of all molecules, but not to inidividual ones.
This means that option C) is FALSE.
Each molecule in gas has its kinetic energy. Option C) is false. All molecules of an ideal gas have the same kinetic energy at a constant temperature.
In a gas, molecules spread out and chaotically collide with each other. The total energy E in the system is always the same, but each particle has its own energy.
On average, all molecules must always have the same kinetic energy in a system. And this average is related to the temperature at which the gas is exposed.
However, each molecule has its own kinetic energy, which differs from the energy of other molecules. It varies according to the direction and velocity they aquire, which continuously changes as they collide. Each molecule in each collision can unpredictably gain or lose energy.
Although, at each moment, molecules have different amounts of energy, the total sum is always E, and most molecules have values close to the average.
The false statement is option C) All molecules of an ideal gas have the same kinetic energy at constant temperature.
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