   Chapter 20, Problem 43GQ

Chapter
Section
Textbook Problem

Chlorine atoms are formed by photochemical reactions of chlorofluorocarbons in the upper atmosphere. Using the average bond energy of the C—Cl bond in Table 8.8, calculate the wavelength of radiation with sufficient energy to break the C—Cl bond. In what region of the electromagnetic spectrum does this fall?

Interpretation Introduction

Interpretation: The wavelength of the radiation with sufficient energy to break C-Cl bond should be calculated and the region where this falls in electromagnetic spectrum should be determined.

Concept introduction:

Electromagnetic radiations are a type of energy surrounding us. They are of different types like radio waves, IR, UV, X-ray etc.

Ultraviolet radiation lies between 200nm to 400nm

Energy associated with a radiation,

Explanation

Given:

From the table 8.8, the average bond energy of C-Cl bond is 339kJ/mol

In-order to find the wavelength of the radiation we can use the equation

E=E=hcλwhereh(Plancksconstant)=6.626×10-34Jsc(speedoflight)=3×108m/s

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