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Ch.6 - Electronic Structure of Atoms
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
All textbooksBrown 15th EditionCh.6 - Electronic Structure of AtomsProblem 104
Chapter 6, Problem 104

The stratospheric ozone (O3) layer helps to protect us from harmful ultraviolet radiation. It does so by absorbing ultraviolet light and falling apart into an O2 molecule and an oxygen atom, a process known as photodissociation. O3(g) → O2(g) + O(g). Use the data in Appendix C to calculate the enthalpy change for this reaction. What is the maximum wavelength a photon can have if it is to possess sufficient energy to cause this dissociation? In what portion of the spectrum does this wavelength occur?

Verified step by step guidance
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Step 1: Identify the reaction and the enthalpy change needed. The reaction is O_3(g) \(\rightarrow\) O_2(g) + O(g). We need to calculate the enthalpy change (\(\Delta\) H) for this reaction using standard enthalpies of formation from Appendix C.
Step 2: Use the formula for the enthalpy change of a reaction: \(\Delta\) H_{reaction} = \(\sum\) \(\Delta\) H_f^{\(\circ\)} (products) - \(\sum\) \(\Delta\) H_f^{\(\circ\)} (reactants). Look up the standard enthalpies of formation for O_3(g), O_2(g), and O(g) in Appendix C.
Step 3: Substitute the values from Appendix C into the enthalpy change formula. Calculate \(\Delta\) H_{reaction} by subtracting the enthalpy of formation of O_3(g) from the sum of the enthalpies of formation of O_2(g) and O(g).
Step 4: To find the maximum wavelength of a photon that can cause this dissociation, use the energy-wavelength relationship: E = \(\frac{hc}{\lambda}\), where E is the energy required (equal to \(\Delta\) H_{reaction} per mole of O_3), h is Planck's constant, c is the speed of light, and \(\lambda\) is the wavelength.
Step 5: Solve for \(\lambda\) (wavelength) by rearranging the equation: \(\lambda\) = \(\frac{hc}{E}\). Calculate \(\lambda\) using the energy value obtained from \(\Delta\) H_{reaction}. Determine the portion of the electromagnetic spectrum this wavelength falls into by comparing it to known ranges (e.g., ultraviolet, visible, etc.).

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Photodissociation

Photodissociation is a process in which a chemical compound breaks down into simpler molecules or atoms upon absorbing light, typically ultraviolet (UV) radiation. In the case of ozone (O3), it absorbs UV light, leading to its dissociation into oxygen molecules (O2) and oxygen atoms (O). This reaction is crucial for understanding how ozone protects the Earth from harmful UV radiation.

Enthalpy Change

Enthalpy change (ΔH) refers to the heat content change of a system at constant pressure during a chemical reaction. It can be calculated using standard enthalpy values from tables, which provide the energy associated with the formation or dissociation of compounds. In this context, calculating the enthalpy change for the photodissociation of ozone helps to understand the energy dynamics involved in the reaction.

Photon Energy and Wavelength

The energy of a photon is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. To cause photodissociation, the photon must have sufficient energy to break the O3 bond, which can be determined by calculating the maximum wavelength that corresponds to this energy. This wavelength typically falls within the ultraviolet region of the electromagnetic spectrum.
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