Problem: It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal. (1 mol electrons = 6.022 x 1023 electrons.) How much energy does it take to remove a single electron from an atom on the surface of solid rubidium? What is the maximum wavelength of light capable of doing this?

🤓 Based on our data, we think this question is relevant for Professor Poehlmann & Waymouth's class at STANFORD.

FREE Expert Solution

Calculate the energy required to remove 1 electron:

E=208.4 kJmol electron×103 J1 kJ×1 mol electron6.022×1023 electron

E = 3.461×10‒19 J/electron



3.461×10‒19 J of energy is required to remove a single electron from an atom on the surface of solid rubidium.


E=cλ=λ·νλν=cλE=hcλ

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Problem Details

It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal. (1 mol electrons = 6.022 x 1023 electrons.) How much energy does it take to remove a single electron from an atom on the surface of solid rubidium? What is the maximum wavelength of light capable of doing this?

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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.

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Based on our data, we think this problem is relevant for Professor Poehlmann & Waymouth's class at STANFORD.

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.