IE = 578.8 KJ/mol
= 578.8 / 6.022*10^23 KJ/atom
= 9.611*10^-22 KJ/atom
= 9.611*10^-19 J/atom
Find the energy supplied by 403 nm:
Given:
lambda = 4.03*10^-7 m
use:
E = h*c/lambda
=(6.626*10^-34 J.s)*(3.0*10^8 m/s)/(4.03*10^-7 m)
= 4.933*10^-19 J
Find energy carried by 2nd wavelength:
E = IE - E1
= 9.611*10^-19 J - 4.933*10^-19 J
= 4.678*10^-19 J
use:
E = h*c/lambda
4.678*10^-19J =(6.626*10^-34 J.s)*(3.0*10^8 m/s)/lambda
lambda = 4.249*10^-7 m
lambda = 425 nm
Answer: 425 nm
In two-photon ionization spectroscopy, the combined energies carried by two different photons are used to remove an ele...
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