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When a problem gives you an energy needed to break a C-C bond in kJ*mol, and asks you for the wavelength required in order to break that bond, do you need to convert that energy in J (by multiplying by 10^3) and then divide it by the Avogadro's number? I am not sure about the moles part (whether you should divide the energy given by 6.022*10^23), because the fact that it is a bond confuses me a little bit.
That is exactly what you do. You're given the energy per mol but you want the total energy which is why you would do that conversion.
Did we ever do this in lecture?
We never did this in lecture, but yes, you divide by Avogadro's number. For that specific question, once you got the energy, you have find the wavelength and then determine if it was in the range of visible light. (visible light being from 400-700 nm)
Is there like a trick or something to memorizing the wavelengths of each light wave? No matter how much I try to remember them, they just seem to slip my mind.
In terms of memorizing the wavelengths, just remember that 400 nm is violet and 700 nm is red. Anything slightly less than 400 nm would be in the UV region. Anything slightly greater than 700 nm is infrared region.
and make sure you know that nm is x 10^-9!