h.w. 1.65  [ENDORSED]

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Emely Reyna 1F
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h.w. 1.65

Postby Emely Reyna 1F » Sun Apr 29, 2018 7:29 pm

the questions asks: 1.65 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?

I'm confused on how I would be able to determine which light could be used? I know I should convert the KJ* mol into J, but what exactly is this value, is it the work function or energy of the photon?

Marisol Sanchez - 1E
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Re: h.w. 1.65

Postby Marisol Sanchez - 1E » Sun Apr 29, 2018 7:52 pm

This value should be the work function because it states that it is the value of energy needed to break the bond, but you could also just use this value as the energy of the photon because it doesn't mention any kinetic energy so that value could be 0 which would make the work function and the energy of the photon equal. After converting the energy you could use the formulas we know to find the wavelength of that energy and see where it falls on the light spectrum.

Chem_Mod
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Re: h.w. 1.65  [ENDORSED]

Postby Chem_Mod » Sun Apr 29, 2018 8:43 pm

You need to convert bond energy in terms of energy per mole of bond to energy per 1 bond. This energy must match the energy of the photon.

This is not related to the work function of a metal.


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