Homework question 1.65


Moderators: Chem_Mod, Chem_Admin

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

Homework question 1.65

Postby alexagreco1A » Sun Apr 15, 2018 9:04 pm

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

Postby Eduardo R 1L » Sun Apr 15, 2018 9:37 pm

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
Posts: 17949
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 406 times

Re: Homework question 1.65

Postby Chem_Mod » Sun Apr 15, 2018 10:24 pm

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.


Return to “Properties of Light”

Who is online

Users browsing this forum: No registered users and 2 guests