It takes 208.4 kj of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal. 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 capable of doing this

Energy: 3.46x10⁻¹⁹ J

Wavelength: 574.0 nm

Explanation:

For the Avogadros' number, we know that 1 mol of electron has 6.02x10²³ electrons, so

6.02x10²³ electrons 208.4 kJ

1 electron x

By a simple direct three rule:

6.02x10²³ x = 208.4

x = 3.46x10⁻²² kJ

Knowing that 1 kJ = 10³ J

E = 3.46x10⁻²²x10³ = 3.46x10⁻¹⁹ J

The energy is related to the wavelenght of the electron by the equation:

E = hxc/λ

Where h is the Planck consant (h = 6.626x10⁻³⁴ m²kg/s), c is the light velocity (c = 3.00x10⁸ m/s), and λ is the wavelenght. So:

3.46x10⁻¹⁹= (6.626x10⁻³⁴x3.00x10⁸)/λ

λ = 5.74x10⁻⁷m

λ = 574.0 nm

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