question_answer

An element undergoes a reaction as shown: \[X+2{{e}^{-}}\xrightarrow{{}}{{X}^{2-}},\] energy released = 30.87 eV/atom. If the energy released, is used to dissociate 4g of \[{{H}_{2}}\] molecules, equally into \[{{H}^{+}}\] and H*, where H* is excited state of H atoms where the electron travels in orbit whose circumference equal to four times its de Broglie's wavelength. Determine the least moles of that would be required. Given: I.E. of H= 13.6eV/atom, bond energy of \[{{H}_{2}}=4.526\]eV/molecule.

Answer:

2