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Jakob Littel

Feb 20, 2025

A mole of red photon of wavelength 725nm has how much KJ?

A mole of red photon of wavelength 725nm has how much KJ?What I did so far...725nm/ 10^9nm = 7. 25 X 10^ -7mE= hc/ wavelength= 1.99 X 10^-25/ 7.25 X 10^-7m = 2.75 X 10^ -19 JThe answer states that it is 165 KJ. Even if I were to convert the number above to KJ it wouldn't be correct.If I were to use E= hvv= c/ wavelength = 3.0 X 10^8 / 7.25 X 10^-7 = 4.14 X 10^ 14E= 6.626 X 10^-34 X 4.14 X 10^ 14 = 2.74 X 10^-19 J.... I don't know why I am not getting the correct answer! please help! also does it matter whether I use E= hc/ wavelength & E=hv (find v through v= c/ wavelength)?Thank you
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Hermina Ferry

Feb 20, 2025

You have successfully completed the first step of the problem which was to compute the energy of a single photon. You simply need to multiply that energy by the number of photons in a mole of photons (6.02E23)If I use your first calculated energy of a photon, 2.75E-19J*6.02E23=166kJ... Show More
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