the kinetic theory leads to the expression = 3/2 kT for the average kinetic energy of a molecule of a gas. the constant k does not depend on the type of molecule. Can this result really be true both for hydrogen and chlorine? (The mass of a hydrogen molecule is about 35 times that of a hydrogen molecule.) Explain why ????

Question

the kinetic theory leads to the expression

<E> = 3/2 kT

for the average kinetic energy of a molecule of a gas. the constant k does not depend on the type of molecule. Can this result really be true both for hydrogen and chlorine? (The mass of a hydrogen molecule is about 35 times that of a hydrogen molecule.) Explain why

????

anonymous · Answer

$$<E > = 3/2 kt$$

cj7529 · Answer

K is constant regardless of the molecule your considering.  So the only quantity that can affect the energy is the temperature.  If you heat hydrogen and chlorine, you will find it much harder to heat the chlorine (its specific heat capacity is over twice that of hydrogen).  


So in terms of energy, you still need to put the extra in (as heat) to get it back out (as kinetic energy of the molecule)