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the bright yellow light emitted by a sodium vapor lamp consists of two emission lines at 589.0 and 589.6 nm. what are the frequency and the energy of a photon of light at each of these wavelengths? what are the enegies in kJ/mol

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  1. c = wavelength x frequency.
    You know c (speed of light is 3 x 10^8 m/s) and you know wavelength (change to meters). Calculate freqency in Herz.
    E = hc/wavelength. That will give you the energy of 1 photon in Joules. Multiply by 6.02 x 10^23 to convert to Joules/mol of photons and change that to kJ/mol. Post your work if you get stuck.

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  5. I believe you should divide by 6.022 x 10^23 moles?

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