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8. Sulfur has a first ionization energy of 1000 kJ/mol. Photons of what frequency are required to ionize one mole of Sulfur?​

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Answer:

the frequency of photons
v = 1.509*10^(39)Hz

Step-by-step explanation:

Given: first ionization energy of 1000 kJ/mol.

No. of moles of sulfur = 1 mole


\Delta E_1 = 1000KJ/mol

We know that plank's constant


h = 6.626*10^(-34) Js

Let the frequency of photons be ν

Also we know that ΔE = hν

this implies ν = ΔE/h


= (10^6J)/(6.626*10^(-34) Js)


v = 1.509*10^(39)Hz

Hence, the frequency of photons
v = 1.509*10^(39)Hz

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