# 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?

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###### FREE Expert Solution

Calculate the energy required to remove 1 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.

$\overline{)\mathbf{E}\mathbf{=}\mathbf{h\nu }}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{c}}{\mathbf{\lambda }}\mathbf{=}\frac{\overline{)\mathbf{\lambda }}\mathbf{·}\mathbf{\nu }}{\overline{)\mathbf{\lambda }}}\phantom{\rule{0ex}{0ex}}\mathbf{\nu }\mathbf{=}\frac{\mathbf{c}}{\mathbf{\lambda }}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{E}\mathbf{=}\frac{\mathbf{hc}}{\mathbf{\lambda }}}$

###### 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?