Problem: 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?

🤓 Based on our data, we think this question is relevant for Professor Huchital's class at FAU.

FREE Expert Solution

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 Js

E=hν

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=λ·νcλ=λ·νλν=cλ

 c = speed of light = 3.0x108 m/s
▪ 
λ = wavelength, m


View Complete Written Solution
Problem Details

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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Photoelectric Effect concept. You can view video lessons to learn Photoelectric Effect. Or if you need more Photoelectric Effect practice, you can also practice Photoelectric Effect practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Huchital's class at FAU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.