Domanda del libro di testo
(b) Use the energy requirements of these two pro- cesses to explain why photodissociation of oxygen is more important than photoionization of oxygen at altitudes below about 90 km.
520
views
Ch.18 - Chemistry of the Environment
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 18, Problema 21b
The wavelength at which the O2 molecule most strongly absorbs light is approximately 145 nm. (b) Would a photon whose wavelength is 145 nm have enough energy to photodissociate O2 whose bond energy is 495 kJ/mol? Would it have enough energy to photoionize O2?
Guida verificata passo dopo passo1
First, understand that photodissociation occurs when a molecule absorbs a photon with enough energy to break a chemical bond. The energy of a photon can be calculated using the formula: E = \( \frac{hc}{\lambda} \), where E is the energy, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and \( \lambda \) is the wavelength in meters.
Convert the given wavelength from nanometers to meters. Since 1 nm = 1 x 10^-9 m, 145 nm is equivalent to 145 x 10^-9 m.
Calculate the energy of a single photon with a wavelength of 145 nm using the formula E = \( \frac{hc}{\lambda} \). Substitute the values for h, c, and \( \lambda \) to find the energy in joules.
Convert the bond energy of O2 from kJ/mol to J/molecule. Since 1 mol contains Avogadro's number of molecules (6.022 x 10^23 molecules/mol), divide the bond energy by Avogadro's number to find the energy required to break one O2 molecule in joules.
Compare the energy of the photon calculated in step 3 with the energy required to break the O2 bond from step 4. If the photon's energy is greater than or equal to the bond energy, it can photodissociate O2. For photoionization, the photon must have even more energy to remove an electron completely, which typically requires more energy than bond dissociation.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
5mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Photon Energy Calculation
The energy of a photon can be calculated using the equation E = hc/λ, where E is energy, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength in meters. For a wavelength of 145 nm, this calculation will determine if the photon has sufficient energy to break molecular bonds or ionize atoms.
Video consigliato:
Percorso guidato
00:41
Moles and Photon Energy
Bond Energy
Bond energy is the amount of energy required to break one mole of bonds in a substance. In this case, the bond energy of O2 is given as 495 kJ/mol, which indicates the energy needed to dissociate the O2 molecule into individual oxygen atoms. Understanding bond energy is crucial for determining whether the energy from the photon is adequate for photodissociation.
Video consigliato:
Percorso guidato
01:50Bond Energy
Photoionization
Photoionization is the process by which an atom or molecule absorbs a photon and subsequently loses an electron, resulting in the formation of a positively charged ion. The energy required for photoionization is typically higher than that needed for photodissociation, making it essential to compare the photon's energy with the ionization energy of O2 to assess if it can cause ionization.
Pratica correlata
Domanda del libro di testo
The ultraviolet spectrum can be divided into three regions based on wavelength: UV-A (315–400 nm), UV-B (280–315 nm), and UV-C (100–280 nm). (b) In the absence of ozone, which of these three regions, if any, are absorbed by the atmo- sphere?
1344
views
Domanda del libro di testo
The ultraviolet spectrum can be divided into three regions based on wavelength: UV-A (315–400 nm), UV-B (280–315 nm), and UV-C (100–280 nm). (a) Photons from which region have the highest energy and therefore are the most harmful to living tissue? (315–400 nm), UV-B (280–315 nm), and UV-C (100–280 nm).
Domanda del libro di testo
(a) Distinguish between photodissociation and photoionization.
2
views
Domanda del libro di testo
The wavelength at which the O2 molecule most strongly absorbs light is approximately 145 nm. (a) In which region of the electromagnetic spectrum does this light fall?
1828
views
Domanda del libro di testo
The ultraviolet spectrum can be divided into three regions based on wavelength: UV-A (315–400 nm), UV-B (280–315 nm), and UV-C (100–280 nm). (c) When appropriate concentrations of ozone are present in the stratosphere, is all of the UV light absorbed before reaching the Earth’s surface? If not, which region or regions are not filtered out?