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?

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.

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

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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?