How would I calculate the energy (in kilojoules) for 1 mole of a photon having a wavelength of 623nm? If I first calculated the energy of the photon in Joules and got 3.20x10^-37J.
I am wondering if I would need to find out the wavelength of 1 mole of these photons first and then carry out the same steps as I did when looking for the energy of the single photon. So:
if I converted nm to m first, then: 6.23x10^11m X 6.022x10^23 = _____m
and plug that into my E= h * c/wavelength = _____ and convert that to kilojoules?
I am wondering if I would need to find out the wavelength of 1 mole of these photons first and then carry out the same steps as I did when looking for the energy of the single photon. So:
if I converted nm to m first, then: 6.23x10^11m X 6.022x10^23 = _____m
and plug that into my E= h * c/wavelength = _____ and convert that to kilojoules?
1 Answer
Your methodology, although not executed, seems sound. However,
Explanation:
Consider,
Moreover, consider the frequency of one photon at that wavelength,
Now, recall,
The energy for one photon of that wavelength is then,
Hence,
of energy are in that many photons of that wavelength.