Question 1.65 (Sixth Edition)


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Steve Magana 2I
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Joined: Fri Sep 28, 2018 12:24 am

Question 1.65 (Sixth Edition)

Postby Steve Magana 2I » Wed Oct 17, 2018 11:50 pm

Question: The energy required to break a C-C bond in a molecule is 348 kJ.mol^-1. Will visible light be able to break this bond? If yes, what is the color of that light? If not, what type of electromagnetic radiation will be suitable?

Does anyone know how to approach this problem? Thank you!

yaosamantha4F
Posts: 31
Joined: Fri Sep 28, 2018 12:29 am

Re: Question 1.65 (Sixth Edition)

Postby yaosamantha4F » Thu Oct 18, 2018 9:12 am

Starting with 348kJ/mol, you would multiply by 348kJ/mol C-C bonds * 1mol C-C bonds/6.022*10^23 C-C bonds *1000J/kJ to ultimately end up 5.78*10^(-19)J as ΔE. You can then use the equation λ=hc/ΔE and plug in Planck's constant, the speed of light, and ΔE to get 3.44*10^-7m (or 344nm). This falls under the range for UV light; visible light therefore is not able to break a C-C bond.


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