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What is the binding energy of an electron in a photosensitive metal (in kj/mol) if the...

What is the binding energy of an electron in a photosensitive metal (in kj/mol) if the minimum frequency of light that can eject from electrons from the metal is 6.3 x 10^-14 Hz?

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Answer #1

Frequency is related to wavelength by the equation:

frequency = speed of light / wavelength

wavelength = speed of light / frequency = (3E8) / (6.3E14) = 1.89E-7 m

Energy is related to wavelength by the equation:

Energy = planck constant * speed of light * wave number

Wave number = 1 / wavelength = 1/1.89E-7 = 5.29E6

Energy = 6.626E-34 * 3E8 * 5.29E6 = 10.5E-19 J

That is the energy of one photon. To convert that to a mole of photons, you multiply by avogadro's constant.

Energy = 10.5E-19 x 6.022E23 = 633241 J / mol

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