We’re being asked to determine the longest wavelength that has enough energy to break the carbon-carbon bonds.
This means we need to determine the wavelength with equivalent energy to break carbon-carbon bonds. This will be the wavelength with an energy of 348 kJ/mol.
Recall that the energy of a photon (E) is given by:
h = Planck’s constant (6.626 × 10–34 J • s)
v = frequency (in s–1)
Also, recall that the frequency (v) and wavelength (λ) are related:
c = speed of light (3.0 × 108 m/s)
Ultraviolet radiation and radiation of shorter wavelengths can damage biological molecules because these kinds of radiation carry enough energy to break bonds within the molecules. A typical carbon-carbon bond requires 348 kJ/mol to break.
What is the longest wavelength of radiation with enough energy to break carbon-carbon bonds?
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