Unformatted text preview: ) Calculate the smallest amount of energy (i.e. one quantum) that an object can absorb from yellow light with a wavelength of 589 nm Energy quantum = h ν so we need to know the frequency ν ν λ = c ν€ = c/ λ ν€ = (3.00 x 10 8 m/s)/(589 x 109 m) ν€ = 5.09 x 10 14 s1 plugging into Planck's equation: E = (6.63 x 1034 Js)*( 5.09 x 10 14 s1 ) E (1 quanta) = 3.37 x 1019 J Note that a quanta is quite small. When we receive infrared radiation from a fireplace we absorb it in quanta according to Planck's Law. However, we can't detect that the energy absorbtion is incremental. On the atomic scale, however, the quantum effects have a profound influence...
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 Fall '10
 LauraChoudry
 Chemistry, pH, Energy, Photon, Light, white hot

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