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valina [46]
3 years ago
5

It takes 498. kJ/mol to break an oxygen-oxygen double bond. Calculate the maximum wavelength of light for which an oxygen-oxygen

double bond could be
broken by absorbing a single photon.
Be sure your answer has the correct number of significant digits.
Chemistry
2 answers:
Neporo4naja [7]3 years ago
5 0

The bond energy required to break the oxygen-oxygen double bond is 240 nm

The energy of the incoming photon = 498 * 10^3 J/mol/6.02 * 10^23 moles = 8.27 * 10^-19 J

Recall that;

E = hc/λ

E = energy of the photon

c = speed of light = 3 * 10^8 m/s

λ = wavelength of photon

h = Plank's constant = 6.63 * 10^-34 Js

λ = hc/E

λ = 6.63 * 10^-34 * 3 * 10^8/8.27 * 10^-19

λ = 2.40 * 10^-7 m

λ = 240 nm

Learn more: brainly.com/question/24302171

Lyrx [107]3 years ago
5 0
  • Energy=498KJ =498×10^3J

We know

\\ \sf\bull\longmapsto E=hv

  • h=planks constant
  • v=frequency

\\ \sf\bull\longmapsto v=\dfrac{E}{h}

\\ \sf\bull\longmapsto v=\dfrac{498\times 10^3J}{6.626\times 10^{-34}Js}

\\ \sf\bull\longmapsto v=75.15\times 10^{37}s^{-1}

\\ \sf\bull\longmapsto v=7.5\times 10^{36}s^{-1}

Now

\\ \sf\bull\longmapsto \lambda=\dfrac{C}{V}

\\ \sf\bull\longmapsto \lambda=\dfrac{3\times 10^{8}ms^{-1}}{7.5\times 10^{36}s^{-1}}

\\ \sf\bull\longmapsto \lambda=2.5\times 10^{-28}m

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