Is at any given temperature the molecules of gases have same kinetic energy?

Answer 1

No. There is a well known distribution of probabilities that describes how likely it is that a given molecule has a given kinetic energy, but a gas will always have some fast and some cold molecule. The average KE is defined by temp, however.

Answer 2

NO - the molecules in a sample of gas are expected to have a Maxwell-Boltzman distribution of velocities. There is a finite probability for molecules to have any particular speed, from zero to near-lightspeed, but the probabilities of those speeds are described by the Maxwell-Boltzman distribution. As the internal energy of the gas increases, the mean velocity increases. In theory all the molecules could have that same mean velocity, but the probability is so incredibly small that even for a very small gas sample you would never expect to observe such a phenomena during the life of the universe.

Answer 3

NO. Depending on there molecular weight it should vary. Heavier gases should have more kinetic energy. But i will like to have second opinion. ( Galileo's experiment of small and big balls falling from height. )

Answer 4

At any given temperature, gas molecules have a range of kinetic energies following a Maxwell-Boltzmann distribution. This means that while the average kinetic energy of the molecules is the same, individual molecules can have different kinetic energies.

Answer 5

As the temperature increases, the kinetic energy of the molecules will increase. As the temperature decreases, the kinetic energy of the molecules will decrease.

Answer 6

False