radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. it is this radiation that causes dyes to fade and your skin to develop a sunburn. if you are bombarded with 1.00 mol of photons with a wavelength of 370. nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to?
Answers
If you are bombarded with 1.00 mol of photons with a wavelength of 370 nm, you are being subjected to 322 kJ/mol of energy.
The energy of a photon is given by the equation:
E = hc/λ
where:
h = Planck's constant = 6.626 x J s
c = speed of light = 2.998 x m/s
λ = wavelength of the radiation
To find the energy of a mole of photons, we need to multiply the energy of a single photon by Avogadro's number (6.022 x ).
First, we need to convert the wavelength of the radiation from nanometers to meters:
370 nm = 370 x m
Now, we can use the equation to calculate the energy of a single photon:
E = hc/λ
E = (6.626 x J s) x (2.998 x
m/s) / (370 x
m)
E = 5.35 x J
Next, we can calculate the energy of a mole of photons:
(5.35 x J/photon) x (6.022 x
photons/mol) = 3.22 x
J/mol
Finally, we can convert the energy to kilojoules per mole of photons:
3.22 x J/mol = 322 kJ/mol
To know more about wavelength refer here
brainly.com/question/31143857#
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