1. The problem statement, all variables and given/known data We know that the average kinetic energy of an ideal gas atom or molecule at Kelvin temperature T is (3/2)kbT. For what temperature T_He does the average kinetic energy of an ideal gas atom or molecule equal the bond energy of the van der Waals bond in He_2 7.9*10^-4 ev? 2. Relevant equations (3/2) kb * T 3. The attempt at a solution 7.9*10^-4 ev * 1.602*10^-19 J = 1.265*10^-22 J (3/2) * kb * 298 K = 1.265*10^-22 J kb = 2.829*10^-25 J The answer asks for a temperature and I have an energy. I was really unsure about this one.