Question

Ozone molecules in the upper atmosphere absorb radiation. If the radiation has a wavelength between 240 nm and 310 nm, the ozone molecules will decompose into oxygen molecules and oxygen atoms. The oxygen atoms then recombine with the oxygen molecules to make more ozone, releasing heat. This converts light energy into heat energy and insulates the Earth. ***** O3(g) → O2(g) + O(g) -> light energy absorbed heat energy released O2(g) + O(g) 03(g) a) What kind of electromagnetic radiation has a wavelength between 240 and 310 nm? b) Which wavelength represents the minimum amount of energy required for this reaction to proceed: 240 nm or 310 nm? c) Calculate the minimum amount of light energy that must be absorbed to convert 1 mole of ozone into oxygen molecules and atoms. Report your answer in kJ/mol. [4 Marks]​

Answer 1

a)ultraviolet rays

Step-by-step explanation:

ultraviolet rays are electromagnetic waves that are found in the range of 240 and 310 somewhere in between the electromagnetic spectrum

b)310nm causes minimum energy because the ultraviolet rays have reacted with oxygen to produce zone

c) 310nm to

=3.1×10^-7m once converted find the frequency using the converted wavelength as your wavelength AND once that has been done find your

E=hv=6.626×10^-34×9.68×10^14=6.414×10^-10J convert J to KJ/MOL will be 386.3KJ/MOL.