Calculate It takes $8.17 \times 10^{-19} \mathrm{J}$ of energy to remove one electron from a gold surface. What is the maximum wavelength of light capable of causing this effect?
Added by Sergio V.
Step 1
We can also express this equation in terms of wavelength, λ, using the equation f = c/λ, where c is the speed of light. Substituting this into the first equation gives E = hc/λ. Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 85 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
It takes $7.21 \times 10^{-19} \mathrm{J}$ of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
600,000+
Students learning Chemistry with Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD
