Calculate the energy, in j, needed to break 1 c-c bond

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The reason there is a danger in exposure to high-energy radiation (e.g., ultraviolet and X rays) is that the radiation can rupture chemical bonds. In some cases, cancer can be caused by it. A carbon-carbon single bond has a bond energy of approximately 348 kJ/mole. What wavelength of light is required to provide sufficient energy to break the C-C bond? In which region of the electromagnetic spectrum is thisCalculate the energy, in J, needed to break 1 C-C bond if it takes 348 kJ to break a mole of C-C bonds.
Enter your response in scientific notation as 1.00e-10, for example.wavelength located?

Reference no: EM131034659

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Calculate the energy, in j, needed to break 1 c-c bond : Enter your response in scientific notation as 1.00e-10, for example.wavelength located?

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