🤓 Based on our data, we think this question is relevant for Professor Lapeyrouse's class at UCF.
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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the The Particle Nature of Light concept. You can view video lessons to learn The Particle Nature of Light. Or if you need more The Particle Nature of Light practice, you can also practice The Particle Nature of Light practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Lapeyrouse's class at UCF.