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

answer

fusion: the energy source of stars. the energy released from the collapse of the gas into a protostar causes the center of the protostar to become extremely hot. when the core is hot enough, nuclear fusion commences. fusion is the process where two hydrogen atoms combine to form a helium atom, releasing energy.

hope it

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