## Homework question 1.65

alexagreco1A
Posts: 34
Joined: Fri Apr 06, 2018 11:03 am

### Homework question 1.65

The energy required to break a C-C bond in a molecule is 348 kJ/mol. 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?

How would I go about solving this after converting this into Joules? How do I know to use lambda=hc/deltaE?

Eduardo R 1L
Posts: 8
Joined: Mon Apr 09, 2018 1:38 pm

### Re: Homework question 1.65

You're right the first step is to convert 348 kj*mol^-1 into only J.
Once you finish the conversion the J you get is the deltaE because it is the energy needed to break the bond.
Now that you have deltaE you can sub it into the equation with the given constants (h,c).
Don't forget to convert the answer to nm so finding the appropriate wavelength on the em spectrum!

Chem_Mod
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### Re: Homework question 1.65

First convert you C-C bond energy in terms of Joules/1 C-C bond. So use Avogadro's number to change moles to per C-C bond. Then since 1 photon interacts with each C-C bond, set hv = the energy value you find and solve for v.