Concept explainers
(a)
Interpretation:
The value of
Concept introduction:
The point at which the bond between the two atoms become nonexistent thus the molecule exists as two separated atoms are known as dissociation limit. The relation between
Where,
•
•
•
•
(b)
Interpretation:
Whether it is expected that
Concept introduction:
The point at which the bond between the two atoms become nonexistent thus the molecule exists as two separated atoms are known as dissociation limit. The relation between
Where,
•
•
•
•
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
Physical Chemistry
- The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?arrow_forwardUsing a table of average bond enthalpies. Table 6.2 ( Sec. 6-6b), estimate the enthalpy change for the industrial synthesis of methanol by the catalyzed reaction of carbon monoxide with hydrogen.arrow_forwardUsing the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forward
- In trichlorofluoromethane refrigerant (CCl3F, also known as Freon-11, R-11, or CFC-11), there are 3 C-Cl bonds. When these are photochemically broken by solar radiation in the stratosphere, free Cl atoms produced can catalytically destroy ozone, O3. If the C-Cl bond energy is 331 kJ/mol, calculate the energy in J to break one C-Cl bond, the frequency of light that corresponds to this photon energy, and the wavelength in nm of this light. What do we call light in this wavelength region? (visible, UV, IR, etc)arrow_forwardUse average bond enthalpies to calculate the enthalpy change for the following gas-phase reaction. CH3OH(g) + HI(g) --> CH3I(g) + H2O(g) ΔHreaction = ?arrow_forwardA scientist studies the bond energies of different compounds containing nitrogen (N). The scientist observes that the N–N bonds in one group of compounds have a bond energy of 209 kJ/mol, while the N–N bonds in another group of compounds have a bond energy of 418 kJ/mol. In one or two sentences, postulate a reason for this difference.arrow_forward
- Acetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forwardlist the following ionic compounds: CsCl, ScN, MgO, LiCl, in order from smallest to largest lattice energy E and explain the order based on the strength of ionic interactions in each compoundarrow_forwardGive only typing answer with explanation and conclusion Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by the following reaction: C(s,graphite)+2H2O(g)→2H2(g)+CO2(g) Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol. Use average bond energies to calculate ΔHrxn for this reaction.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning