An X-ray photon with a wavelength of 0.933 nm strikes a surface. The emitted electron has a kinetic energy of 994 eV .
What is the binding energy of the electron in kJ/mol? [Note that KE = 1/2mv^2 and 1 electron volt (eV) = 1.602×10^−19J.]
KE = 994 eV
= 994 * 1.602*10^-19 J
= 1.59*10^-16 J
Given:
lambda = 9.33*10^-10 m
use:
E = h*c/lambda
=(6.626*10^-34 J.s)*(3.0*10^8 m/s)/(9.33*10^-10 m)
= 2.131*10^-16 J
Use:
Eo = E - KE
= 2.131*10^-16 J - 1.59*10^-16 J
= 5.41*10^-17 J
This is bonding energy for 1 electron
For 1 mol of electron
Eo = 6.022*10^23 * 5.41*10^-17 J/mol
= 3.26*10^7 J/mol
= 3.26*10^4 KJ/mol
Answer: 3.26*10^4 KJ/mol
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