What is the Maximum Wavelength of Light to Remove Electrons from Rubidium?

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To determine the maximum wavelength of light capable of removing electrons from rubidium, the energy required is 208.4 kJ per mole, which translates to an energy of 3.461e-19 J for a single electron. Using the equation E = hc/lambda, where h is Planck's constant (6.626e-34 J·s) and c is the speed of light (2.9979e8 m/s), the wavelength can be calculated. The correct approach involves using the energy per photon to find the corresponding wavelength. This method clarifies the relationship between photon energy and wavelength for electron removal in rubidium.
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Homework Statement


It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal.
What is the maximum wavelength of light capable of doing this?

Homework Equations


Ephotons=hc/lambda



The Attempt at a Solution


I don't know the energy of the photon. I know h=6.626e-34, c=2.9979e8
I'm trying to find lambda but w/o the Ephoton I don't how to solve the equation.I found the energy to remove a single electron which is 3.461e-19.
 
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If you assume that the 208.4kJ was from identical wavelength photons of just the minimum energy to remove the electron, you could work out the energy per photon then use E = hc/lambda to work out the wavelength.
 
Thank You, I was using the wrong energy.
 
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