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binding energy of an electron in KJ/mol.?
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The energy of the photon is
E_photon = h∙c / λ
= h∙c / λ
= 4.1357×1015eVs ∙ 3.0×10+8m/s / 0.947×109m.
= 1310eV
The binding energy of a single electron equals the difference of the photon energy and the energy of the emitted electron
E_bind = E_photon – E_kin
= 1310eV – 985eV
= 325eV
= 5.207×1017J
So thew binding energy of mole of electron is
E_bind = 5.207×1017J ∙ 6.022×1017mol⁻¹
= 31357J/mol
= 31.357kJ/mol

Binding Energy Of Electron

Electron Binding Energy

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RE:
binding energy of an electron in KJ/mol.?
An Xray photon of wavelength 0.947nm strikes a surface. The emitted electron has a kinetic energy of 985eV . what is the binding energy of the electron in KJ/mol

There seems to be some confusion in the calculations.
Ephoton=h∙c/λ
=(6.626×10^34J∙s)∙(3.00×10^8m/s)/(9.47×10^10m)
This is the basic setup^
Before you calculate it, convert Planck’s constant into eV
(6.626×10^34J∙s)/(1.602×10^19J)
=4.136×10^15eVs
Now use this in lieu of Planck’s constant in the equation
(4.136×10^15eVs)(3.00×10^8m/s)/(9.47×10^10m)
=1310eV
Now Ebind= Ephoton – Ekinetic
=1310eV985eV
=325eV
Now use the conversion factor for eV to J (Could be given in problem or not) but regardless it’s 1eV=1.602×10^19J
(325)(1.602×10^19J)=5.2065×10^17J
Convert to J/mol by multiplying by Avagodro’s number
(5.207×10^17)(6.022×10^23)
=31353543J/mol (divide by 1000)
=31353kJ/mol or (3.14×10^4kJ/mol)
Hope this helped!
Source(s): College Student 
divide by 1000. 1kj = 1000 j
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