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dexar [7]
3 years ago
5

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 108 m/s; h = 6

.63 × 10–34 J • s; NA = 6.022 × 1023 moles–1)
Chemistry
1 answer:
ASHA 777 [7]3 years ago
4 0

<u>Answer:</u> The energy of a mole of photons is 2.46\times 10^{5}J

<u>Explanation:</u>

The relation between energy and wavelength of light is given by Planck's equation, which is:

E=\frac{N_Ahc}{\lambda}

where,  

E = energy

h = Planck's constant  = 6.626\times 10^{-34}Js

c = speed of light  = 3.0\times 10^8m/s

N_A =  Avogadro's number = 6.022\times 10^{23}

\lambda = wavelength of photon = 486 nm = 486\times 10^{-9}m     (Conversion factor:  1m=10^9nm )

Putting values in above equation, we get:  

E=\frac{6.022\times 10^{23}\times 6.626\times 10^{-34}Js\times 3.0\times 10^8m/s}{486\times 10^{-9}m}\\\\E=2.46\times 10^{5}J/mol

Hence, the energy of a mole of photons is 2.46\times 10^{5}J

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