Question

1. Chlorofluorocarbons (CFCs) A carbon-chlorine bond in the CFC molecule can be broken by sunlight, leaving a highly reactive free radical which then goes on to destroy the surrounding ozone molecules. The energy of a C-Cl bond is 328 kJ/mole. Calculate the wavelength of light needed to break a bond in a single molecule. In which region of the spectrum (infrared, visible, UV) does this wavelength fall

Answer 1

Answer: The wavelength for this photon is 365 nm. The wavelength corresponds to UV region.

Explanation:

The relationship between wavelength and energy of the wave follows the equation:

$E=\frac{Nhc}{\lambda}$

E= energy

N = avogadros number

$\lambda$ = wavelength of the wave

h = Planck's constant  = $6.626\times 10^{-34}Js$

c = speed of light = $3\times 10^8m/s$

$328\times 10^3J=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}\times 3\times 10^8m/s}{\lambda}$

$\lambda=3.65\times 10^{-7}m=365nm$   $1m=10^9nm$

Thus wavelength for this photon is 365 nm. The wavelength of 365 nm corresponds to UV region.