Chemistry
12th Edition
ISBN: 9780078021510
Author: Raymond Chang Dr., Kenneth Goldsby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 9, Problem 9.122QP
Experiments show that it takes 1656 kJ/mol to break all the bonds in methane (CH4) and 4006 kJ/mol to break all the bonds in propane (C3H8). Based on these data, calculate the average bond enthalpy of the C─C bond.
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Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction:
2co(g) + 2NO(g)→2C02(g) + N2(g)
kJ
The average bond enthalpy for C−H is 413 kJ/mol. 413 kJ of energy is required to break a mole of CH into atoms: CH(g)→C(g)+H(g), ΔH=413 kJ Using this information, and your answer from Part A, calculate the enthalpy change of the reaction from Part B. That is, calculate the energy required to break only the carbon-carbon bonds in benzene. PART A ANSWER ΔH∘rxn =
5535.1 kJ.. PART B ANSWER C6H6(g)→6CH(g)
Use average bond energies together with the standard enthalpy of formation of C( g) (718.4 kJ/mol) to estimate the standard enthalpy of formation of gaseous benzene, C6H6( g). (Remember that average bond energies apply to the gas phase only.) Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene,82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?
Chapter 9 Solutions
Chemistry
Ch. 9.1 - Prob. 1RCCh. 9.2 - Use Lewis dot symbols to represent the formation...Ch. 9.2 - Use Lewis dot symbols to represent the formation...Ch. 9.3 - Which of the following compounds has a larger...Ch. 9.4 - Why is it not possible for hydrogen to form double...Ch. 9.5 - Which of the following bonds is covalent, which is...Ch. 9.5 - Identify the electrostatic potential maps shown...Ch. 9.6 - Write the Lewis structure for carbon disulfide...Ch. 9.6 - Write the Lewis structure for formic acid (HCOOH).Ch. 9.6 - Write the Lewis structure for the nitrite ion...
Ch. 9.6 - The molecular model shown here represents guanine,...Ch. 9.7 - Write formal charges for the nitrite ion (NO2).Ch. 9.7 - Draw the most reasonable Lewis structure of a...Ch. 9.7 - Consider three possible atomic arrangements for...Ch. 9.8 - Draw three resonance structures for the...Ch. 9.8 - The molecular model shown here represents...Ch. 9.9 - Prob. 9PECh. 9.9 - Prob. 10PECh. 9.9 - Prob. 11PECh. 9.9 - Write the Lewis structure of sulfur tetrafluoride...Ch. 9.9 - Both boron and aluminum tend to form compounds in...Ch. 9.10 - Calculate the enthalpy of the reaction...Ch. 9.10 - For the reaction H2(g)+C2H4(g)C2H6(g) (a) Estimate...Ch. 9.10 - Why does Hrxn calculated using bond enthalpies not...Ch. 9 - What is a Lewis dot symbol? To what elements does...Ch. 9 - Use the second member of each group from Group 1A...Ch. 9 - Prob. 9.3QPCh. 9 - Write Lewis dot symbols for the following ions:...Ch. 9 - Write Lewis dot symbols for the following atoms...Ch. 9 - Explain what an ionic bond is.Ch. 9 - Prob. 9.7QPCh. 9 - Name five metals and five nonmetals that are very...Ch. 9 - Name one ionic compound that contains only...Ch. 9 - Name one ionic compound that contains a polyatomic...Ch. 9 - Prob. 9.11QPCh. 9 - In which of the following states would NaCl be...Ch. 9 - Prob. 9.14QPCh. 9 - An ionic bond is formed between a cation A+ and an...Ch. 9 - Prob. 9.16QPCh. 9 - Use Lewis dot symbols to show the transfer of...Ch. 9 - Prob. 9.18QPCh. 9 - For each of the following pairs of elements, state...Ch. 9 - Prob. 9.20QPCh. 9 - What is lattice energy and what role does it play...Ch. 9 - Explain how the lattice energy of an ionic...Ch. 9 - Specify which compound in the following pairs of...Ch. 9 - Compare the stability (in the solid state) of the...Ch. 9 - Use the Born-Haber cycle outlined in Section 9.3...Ch. 9 - Calculate the lattice energy of calcium chloride...Ch. 9 - What is Lewiss contribution to our understanding...Ch. 9 - Use an example to illustrate each of the following...Ch. 9 - What is the difference between a Lewis dot symbol...Ch. 9 - How many lone pairs are on the underlined atoms in...Ch. 9 - Compare single, double, and triple bonds in a...Ch. 9 - Compare the properties of ionic compounds and...Ch. 9 - Define electronegativity, and explain the...Ch. 9 - List the following bonds in order of increasing...Ch. 9 - Arrange the following bonds in order of increasing...Ch. 9 - Four atoms are arbitrarily labeled D, E, F, and G....Ch. 9 - List the following bonds in order of increasing...Ch. 9 - Classify the following bonds as ionic, polar...Ch. 9 - Classify the following bonds as ionic, polar...Ch. 9 - Prob. 9.41QPCh. 9 - 9.42 Explain the concept of formal change. Do...Ch. 9 - Write Lewis structures for the following molecules...Ch. 9 - Write Lewis structures for the following molecules...Ch. 9 - Write Lewis structures for the following...Ch. 9 - Write Lewis structures for the following...Ch. 9 - The following Lewis structures for (a) HCN, (b)...Ch. 9 - The skeletal structure of acetic acid shown here...Ch. 9 - Define bond length, resonance, and resonance...Ch. 9 - Is it possible to trap a resonance structure of a...Ch. 9 - Write Lewis structures for the following species,...Ch. 9 - Draw three resonance structures for the chlorate...Ch. 9 - Write three resonance structures for hydrazoic...Ch. 9 - Draw two resonance structures for diazomethane,...Ch. 9 - Draw three resonance structures for the molecule...Ch. 9 - Draw three reasonable resonance structures for the...Ch. 9 - Why does the octet rule not hold for many...Ch. 9 - Give three examples of compounds that do not...Ch. 9 - Because fluorine has seven valence electrons...Ch. 9 - What is a coordinate covalent bond? Is it...Ch. 9 - Prob. 9.61QPCh. 9 - In the vapor phase, beryllium chloride consists of...Ch. 9 - Of the noble gases, only Kr, Xe, and Rn are known...Ch. 9 - Write a Lewis structure for SbCl5. Does this...Ch. 9 - Prob. 9.65QPCh. 9 - Write Lewis structures for the reaction...Ch. 9 - What is bond enthalpy? Bond enthalpies of...Ch. 9 - Explain why the bond enthalpy of a molecule is...Ch. 9 - From the following data, calculate the average...Ch. 9 - For the reaction O(g)+O2(g)O3(g)H=107.2kJ/mol...Ch. 9 - The bond enthalpy of F2(g) is 156.9 kJ/mol....Ch. 9 - For the reaction 2C2H6(g)+7O2(g)4CO2(g)+6H2O(g)...Ch. 9 - Prob. 9.73QPCh. 9 - Which of the following are ionic compounds? Which...Ch. 9 - Prob. 9.75QPCh. 9 - Use ionization energy (see Table 8.2) and electron...Ch. 9 - Prob. 9.78QPCh. 9 - Prob. 9.79QPCh. 9 - Write three reasonable resonance structures for...Ch. 9 - Prob. 9.81QPCh. 9 - Give an example of an ion or molecule containing...Ch. 9 - Draw four reasonable resonance structures for the...Ch. 9 - Prob. 9.84QPCh. 9 - Draw reasonable resonance structures for the...Ch. 9 - Are the following statements true or false? (a)...Ch. 9 - Prob. 9.87QPCh. 9 - Using the following information and the fact that...Ch. 9 - Prob. 9.89QPCh. 9 - Which of the following molecules has the shortest...Ch. 9 - Most organic acids can be represented as RCOOH,...Ch. 9 - Which of the following species are isoelectronic:...Ch. 9 - The following species have been detected in...Ch. 9 - The amide ion, NH2, is a Brnsted base. Represent...Ch. 9 - Draw Lewis structures for the following organic...Ch. 9 - The triiodide ion (I3) in which the I atoms are...Ch. 9 - Compare the bond enthalpy of F2 with the energy...Ch. 9 - Methyl isocyanate (CH3NCO) is used to make certain...Ch. 9 - Prob. 9.99QPCh. 9 - Prob. 9.100QPCh. 9 - Prob. 9.101QPCh. 9 - Draw Lewis structures for the following...Ch. 9 - Prob. 9.103QPCh. 9 - Prob. 9.104QPCh. 9 - Draw Lewis structures for the following organic...Ch. 9 - Write Lewis structures for the following four...Ch. 9 - Prob. 9.107QPCh. 9 - Prob. 9.108QPCh. 9 - Write three resonance structures for (a) the...Ch. 9 - (a) From the following data calculate the bond...Ch. 9 - Prob. 9.111QPCh. 9 - What are the other two reasons for choosing (b) in...Ch. 9 - Prob. 9.113QPCh. 9 - The NO bond distance in nitric oxide is 115 pm,...Ch. 9 - Prob. 9.115QPCh. 9 - Prob. 9.116QPCh. 9 - Prob. 9.117QPCh. 9 - Prob. 9.118QPCh. 9 - Draw a Lewis structure for nitrogen pentoxide...Ch. 9 - In the gas phase, aluminum chloride exists as a...Ch. 9 - The hydroxyl radical (OH) plays an important role...Ch. 9 - Experiments show that it takes 1656 kJ/mol to...Ch. 9 - Calculate Hrxn at 25C of the reaction between...Ch. 9 - Calculate Hrxn at 25C of the reaction between...Ch. 9 - Draw three resonance structures of sulfur dioxide...Ch. 9 - Vinyl chloride (C2H3Cl) differs from ethylene...Ch. 9 - Prob. 9.127QPCh. 9 - The American chemist Robert S. Mulliken suggested...Ch. 9 - Prob. 9.129QPCh. 9 - A student in your class claims that magnesium...Ch. 9 - Shown here is a skeletal structure of borazine...Ch. 9 - Calculate the wavelength of light needed to carry...Ch. 9 - Prob. 9.133QPCh. 9 - From the lattice energy of KCl in Table 9.1 and...Ch. 9 - The species H3+ is the simplest polyatomic ion....Ch. 9 - The bond enthalpy of the CN bond in the amide...Ch. 9 - In 1999 an unusual cation containing only nitrogen...Ch. 9 - Nitroglycerin, one of the most commonly used...Ch. 9 - Give a brief description of the medical uses of...Ch. 9 - Prob. 9.140QPCh. 9 - The isolated O2 ion is unstable so it is not...Ch. 9 - When irradiated with light of wavelength 471.7 nm,...Ch. 9 - Recall from Chapter 8 that the product of the...Ch. 9 - The reaction between fluorine (F2) with ethane...Ch. 9 - A new allotrope of oxygen, O4, has been reported....Ch. 9 - Because bond formation is exothermic, when two...Ch. 9 - Estimate Hf for sodium astatide (NaAt) according...
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- Using 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_forwardWrite all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardUsing the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forward
- Estimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) 3CH2CH3(g) The enthalpies of formation for C6H6(g) and C6H12 (g) are 82.9 and 90.3 kJ/mol. respectively. Calculate H for the two reactions using standard enthalpies of formation from Appendix 4. Account for any differences between the results obtained from the two methods.arrow_forwardA commercial process for preparing ethanol (ethyl alcohol), C2H5OH, consists of passing ethylene gas. C2H4, and steam over an acid catalyst (to speed up the reaction). The gas-phase reaction is Use bond enthalpies (Table 9.5) to estimate the enthalpy change for this reaction when 37.0 g of ethyl alcohol is produced.arrow_forwardCompare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?arrow_forward
- hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?arrow_forwardConsider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forwardhat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?arrow_forward
- Acetylene gas (ethyne; HC≡CH) burns with oxygen in an oxyacetylene torch to produce carbon dioxide, water vapor, and the heat needed to weld metals. The heat of combustion for acetylene is −1259 kJ/mol. Calculate the C≡C bond energy. The average bond energies (kJ/mol) C―H 413 C―C 347 C═C 620 H―H 436 O―O 142 O═O 498 H―O 467 C―O 351 C═O 799arrow_forwardBased on the bond energies for the reaction below, what is the enthalpy of the reaction? HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (g)arrow_forwardCalculate the enthalpy change (ΔH(rxn)) of the following reaction using the bond energies above. Draw the correct Lewis structures to determine the bonding structure. Calculate reactant energy – product energy for your final answer. H2 (g) + CO2 (g) → H2O (g) + CO (g)arrow_forward
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