Calculate the energy of a single photon in joules and the energy of a mole of ph

Question

Calculate the energy of a single photon in joules and the energy of a mole of photons in J/mol for light having wavelengths of 10 m (radio and TV waves). 10.0 cm (microwaves), 10 microns (infrared range), 550 nm (green light), 300 nm (ultraviolet), and 1.00 A (X rays). Do these numbers explain the relative danger of electromagnetic radiation of differing wavelengths? The de Broglie equation for a particle can be applied to an electron orbiting a nucleus if one assumes that the electron must have an exact integral number of wavelengths as it covers the circumference of the orbit having radius r: n lambda = 2 pi r. From this, derive Bohr's quantized angular momentum postulate.

Explanation / Answer

4)
for wavelength = 10 m

energy of 1 photon = h*c/wavelength
= (6.626*10^-34)*(3*10^8)/(10)
= 1.99*10^-26 J

energy of 1 mol = energy of 1 photon * Avogadro's number
= 1.99*10^-26 * 6.022*10^23
=0.012 J/mol

similarly do it for all the wavelength
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as wavelength decreases, energy will increase and relative danger increases

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