Solved: We know from Chapter 18 that the average kinetic

QUESTION:

We know from Chapter 18 that the average kinetic energy of an ideal-gas atom or molecule at Kelvin temperature  is \(\frac{3}{2} K T\) For what value of  does this energy correspond to (a) the bond energy of the van der Waals bond in \(\mathrm{He}_{2}\left(7.9 \times 10^{-4} \mathrm{eV}\right)\) and
(b) the bond energy of the covalent bond in \(H_{2}(4.48 e V) ?\) (c) The kinetic energy in a collision between molecules can go into dissociating one or both molecules, provided the kinetic energy is higher than the bond energy. At room temperature , is it likely that \(\mathrm{He}_{2}\) molecules will remain intact after a collision? What about \(H_{2}\) molecules? Explain.

Equation transcription:

Text transcription:

frac{3}{2} K T

{He}{2}(7.9 \times 10^{-4} eV})

H{2}(4.48 e V) ?

{He}{2}

H{2}