Consider equimolar samples of different ideal gases at the same volume and temperature. Gas A has a higher molar mass than gas B. Compare the pressures. Compare the rms speeds. Compare the average kinetic energies. A > B A > B A > B A = B A = B A = B A D C = D C D C = D C D C = D C F E = F E F E = F E F E = F E
The molecules of an ideal gas are relatively very far apart on the average.
B.
At a given temperature, according to the kinetic molecular theory, the average velocity of He atoms is the same as the average velocity of F2 molecules.
C.
The average kinetic energies of molecules of samples of different ideal gases at the same temperature are the same.
D.
The molecules of a gas move in straight paths until they collide with other molecules or the walls of their containers, according to the kinetic molecular theory.
