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.

Step-by-step explanation:

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

`E=(Nhc)/(\lambda)`

E= energy

N = avogadros number

`\lambda` = wavelength of the wave

h = Planck's constant =
`6.626* 10^(-34)Js`

c = speed of light =
`3* 10^8m/s`

`328* 10^3J=(6.023* 10^(23)* 6.626* 10^(-34)* 3* 10^8m/s)/(\lambda)`

`\lambda=3.65* 10^(-7)m=365nm`
`1m=10^9nm`

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