Need help on ozone chemistry anyone?

[rushuk]

Homework Statement

Ozone dissociate according to this reaction

O3 ---> O2 + O /_\H = +106.4KJmol-1

(1) Calculate how much energy is required in Joules to dissociate a single molecule of ozone?

(2) Determine the wavelenght of light that has this energy. What region of the electro magnetic spectrum does this correspond to?

(3) Does light of this wavelenght actually cause the dissociation of ozone? explain your answer.

Na= L = 6.022x10^23


i would really appreciate help with this or an understanding - I've understood the atmospheric topics but can't get my head around this!

thanks

Homework Equations

The Attempt at a Solution

 

[Nino MMP]

(1) Energy required to dissociate a single molecule of ozone = 106.4 KJmol-1 x 6.022x10^23 molecules = 6.35x10^25 J. (2) Wavelength = hc/E= 6.63x10^-34 x 3x10^8 / 6.35x10^25 = 5.43x10^-7 m. This corresponds to the ultraviolet region of the electromagnetic spectrum.(3) Yes, light of this wavelength does cause the dissociation of ozone. This is because the frequency of ultraviolet light is sufficient to provide the energy required to break the bonds in the ozone molecule and cause it to dissociate into oxygen and oxygen atoms.