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Wavelength of light required to break C-C, C-Cl & O=O bonds

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Without stratospheric ozone (O3), harmful solar radiation would cause gene alterations. Ozone forms when O2 breaks and each O atom reacts with another O2 molecule. It is destroyed by reaction with Cl atoms formed when the C-Cl bond in synthetic chemicals breaks. Find the wavelengths of light that can break the C-Cl bond AND the bond in O2. 2. Carbon-carbon bonds form the 'backbone' of nearly every organic and biological molecule. The average bond energy of the C-C bond is 347 kJ/mol. Calculate the frequency and wavelength of the least energetic photon that can break an average C-C bond. In what region of the electromagnetic spectrum is this radiation?

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Solution Summary

The solution shows how to obtain the wavelength of light required to break a bond of a given energy.

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1. Without stratospheric ozone (O3), harmful solar radiation would cause gene alterations. Ozone forms when O2 breaks and each O atom reacts with another O2 molecule. It is destroyed by reaction with Cl atoms formed when the C-Cl bond in synthetic chemicals breaks. Find the wavelengths of light that can break the C-Cl bond AND the bond in O2.

The C-Cl bond has an energy of 339 kJ/mol, the O=O bond has an energy of 498 kJ/mol.
The formula used here ...

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