## 1.65 : Will visible light be able to break C-C bond? [ENDORSED]

$E=hv$

Nhi Vo 3A
Posts: 50
Joined: Sat Jul 09, 2016 3:00 am

### 1.65 : Will visible light be able to break C-C bond?

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 the light? If not, what type of electromagnetic radiation will be suitable?

Also, how do I convert from kj/mol to just joules?

Thank you

Jessica Huang 1M
Posts: 26
Joined: Wed Sep 21, 2016 2:59 pm

### Re: 1.65 : Will visible light be able to break C-C bond?  [ENDORSED]

Converting kJ/mol to joules:

348 kJ/mol * (1000 J/ 1 kJ) * (1 mol of C-C bonds/6.022x10^23 C-C bonds) = 5.78x10^-19 J

Plug 5.78x10^-19 J for E in the equation E=hc/(lamda).

Solve for lamda.

You would get 3.44x10^-7 m or 344 nm.

Visible light wavelength is within the range of 700nm and 400 nm. Therefore, visible light cannot break the C-C bond.