Asked by Dom
Problem:
What wavelength photon would be required to ionize a hydrogen atom in the ground state and give the ejected electron a kinetic energy of 19.1 eV ?
Answer--> λ =______nm
[Note: I got 3.8x10^-8. I got it wrong twice]
My steps:
(32.7 eV)(1.6x10^19)= 52.32x10^-19
Next I did this:
((6.626x10^-34)(3x10^8m/s))/(52.32x10^-19)=3.8x10^-8
My answer--> 3.8⋅10^−8
What wavelength photon would be required to ionize a hydrogen atom in the ground state and give the ejected electron a kinetic energy of 19.1 eV ?
Answer--> λ =______nm
[Note: I got 3.8x10^-8. I got it wrong twice]
My steps:
(32.7 eV)(1.6x10^19)= 52.32x10^-19
Next I did this:
((6.626x10^-34)(3x10^8m/s))/(52.32x10^-19)=3.8x10^-8
My answer--> 3.8⋅10^−8
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