We are asked to calculate the maximum wavelength of light that takes takes 7.21 x 10 -19 J of energy to remove an electron from an iron atom
Calculate the wavelength from the total energy (ΔE).
• ΔE = 7.21 x 10 -19 J
• h = 6.626x10-34 J∙s
In the equation, the frequency of the light is used but we need wavelength. We can relate frequency and wavelength using the speed of light:
▪ c = speed of light = 3.0x108 m/s
▪ λ = wavelength, m
It takes 7.21 x 10 -19 J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.