Question

Two containers hold an ideal gas at the same temperature and pressure. Both containers hold the same type of gas, but container B has twice the number of particles and twice the volume of container A. The average kinetic energy per molecule in container B is :
A. Twice that for container A

B. The same as that for container A

C. Half that for container A

D. Impossible to determine

Answer 1

Answer:

B. The same as that for container A

Explanation:

To calculate the average Kinetic Energy per molecule,

$K_{avg} = 3/2 K_{B} T$

Where $K_{avg}$ is the average kinetic energy per molecule and $K_{B}$ is the Boltzmann constant

From the above equation it is seen that $K_{avg}$ only depends on the temperature of the gas

And since the temperatures of both gases are equal, their average kinetic energy per molecule is the same