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An element undergoes a reaction as shown, X+2e- --------> X2- Energy released=30.87eV/atom.If the energy released is used to dissociate 4g of H2 molecules,equally into H+ and H*, where H* is the excited state of H atoms where the electron travels in orbit whose circumference equal to four times it's de Brogllie's wavelength.Determine the least moles of X that would be required: Given I.E.of H=13.6eV/atom,bond energy of H2 =4.526eV/molecule.

An element undergoes a reaction as shown,
            X+2e- --------> X2-
Energy released=30.87eV/atom.If the energy released is used to dissociate 4g of H2 molecules,equally into H+ and H*, where H* is the excited state of H atoms where the electron travels in orbit whose circumference equal to four times it's de Brogllie's wavelength.Determine the least moles of X that would be required:
Given I.E.of H=13.6eV/atom,bond energy of H2 =4.526eV/molecule.
 

Grade:12th pass

1 Answers

Avni Chauhan
askIITians Faculty 247 Points
5 years ago
Here, each molecule of H2

1.)dissociates (this requires bond dissociation enthalpy) into

2)H+(for which we require ionization enthalpy) and

3)H*(which is the excited H atom)
this atom is in the fourth state. Energy in this state = 13.6/n2= 13.6/16
therefore energy supplied = 13.6 – (13.6/16) = (15/16) 13.6

And we have a total of 4g H2molecules means 2Namolecules
Therefore energy required =
= 2 * 6.022*1023(B.D.E + I.E. + energy for excitation)

=2 * 6.022*1023 (4.526 + 13.6 + (15/16) 13.6)

= (2 * 6.022*1023* 30.876) eV
This energy is supplies by atoms of X. Energy released per atom = 30.87eV /atom
so, atoms required = 2* 6.022*1023= 2 moles

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