question of the photon energy?
I tried a few things and have yet to get the right answer. So any help would be appreciated. The bright red color of the highway safety flares comes from strontium ions in salts such as Sr (NO3) 2 and SrCO3. Burning an outbreak occurs ions strontium in the excited states, which then emit red photons at 606 nm and several wavelengths between 636 and 688 nm. Calculate the energy emitted if one mole of strontium ions undergo transition at 606 nm. Thanks
We have to use a pair of equations (which, no doubt, have tried), and right units to use E = hc / λ h Planck's constant = 6.64 x 10 ^ -34 Js Speed of light c = 3.00 x 10 ^ 8 m / s wavelength of light = 606 nm = 6.06 x 10 ^ -7 m So , the energy of a photon of 606 nm: E = hc / λ = (6.64 x 10 ^ -34 Js) (3.00 x 10 ^ 8 m / S) / (6.06 x 10-7 m) = 3.29 x 10 ^ — 19 J If we had a mole of strontium atoms, that would 3.29 x 10 ^ -19 J / atom x 6.023 x 10 ^ 23 atoms = 1.98 x 10 ^ 5 J or 198 kJ. I hope that helped!
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