Principles of Chemistry: A Molecular Approach (3rd Edition)
3rd Edition
ISBN: 9780321971944
Author: Nivaldo J. Tro
Publisher: PEARSON
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Textbook Question
Chapter 9, Problem 14SAQ
Use bond energies to determine
a. -1549 kJ
b. 1549 kJ
c. -l2 kJ
d. 12 kJ
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Use bond energies to determine ΔHrxn for the reaction between ethanol and hydrogen chloride.
CH3CH2OH(g)+HCl(g)→CH3CH2Cl(g)+H2O(g)
Average Bond Energies
Bond
Bond Energy (kJ/mol)
H−C
414
H−O
464
H−F
565
H−Cl
431
H−Br
364
C−Cl
339
C−O
360
Cl−F
253
Cl−Cl
243
Br−Cl
218
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation
NH3 (g) + 2 O2 (g) --> HNO3 (g) + H20 (g)
Average molar bond enthalpies. (?bond)
Bond
??⋅???−1
Bond
??⋅???−1
O−H
464
C≡N
890
O−O
142
N−H
390
C−O
351
N−O
201
O=O
502
N=N
418
C=O
730
N=O
607
C−C
347
F−F
155
C=C
615
Cl−Cl
243
C≡C
811
Br−Br
192
C−H
414
H−H
435
C−F
439
H−F
565
C−Cl
331
H−Cl
431
C−Br
276
H−Br
368
C−N
293
H−S
364
C=N
615
S−S
225
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔHrxn∘ for the equation
CCl4(g)+2F2(g)⟶CF4(g)+2Cl2(g)CCl4(g)+2F2(g)⟶CF4(g)+2Cl2(g)
The bonding in the molecules is shown.
Average molar bond enthalpies (?bond)(Hbond)
Bond
??⋅???−1kJ⋅mol−1
Bond
??⋅???−1kJ⋅mol−1
O−HO−H
464464
C≡NC≡N
890890
O−OO−O
142142
N−HN−H
390390
C−OC−O
351351
N−NN−N
159159
O=OO=O
502502
N=NN=N
418418
C=OC=O
730730
N≡NN≡N
945945
C−CC−C
347347
F−FF−F
155155
C=CC=C
615615
Cl−ClCl−Cl
243243
C≡CC≡C
811811
Br−BrBr−Br
192192
C−HC−H
414414
H−HH−H
435435
C−FC−F
439439
H−FH−F
565565
C−ClC−Cl
331331
H−ClH−Cl
431431
C−BrC−Br
276276
H−BrH−Br
368368
C−NC−N
293293
H−SH−S
364364
C=NC=N
615615
S−SS−S
225
Chapter 9 Solutions
Principles of Chemistry: A Molecular Approach (3rd Edition)
Ch. 9 - Prob. 9.1PCh. 9 - Arrange the compounds in order or increasing...Ch. 9 - Prob. 9.2MPCh. 9 - Prob. 9.3PCh. 9 - Prob. 9.4PCh. 9 - Prob. 9.5PCh. 9 - Prob. 9.6PCh. 9 - Prob. 9.7PCh. 9 - Prob. 9.8PCh. 9 - Prob. 9.8MP
Ch. 9 - Prob. 9.9PCh. 9 - Write the Lewis structure for XeF4.Ch. 9 - Prob. 9.10MPCh. 9 - Prob. 9.11PCh. 9 - Prob. 9.11MPCh. 9 - Prob. 1SAQCh. 9 - Prob. 2SAQCh. 9 - Prob. 3SAQCh. 9 - Prob. 4SAQCh. 9 - Prob. 5SAQCh. 9 - Prob. 6SAQCh. 9 - Prob. 7SAQCh. 9 - Prob. 8SAQCh. 9 - Prob. 9SAQCh. 9 - Prob. 10SAQCh. 9 - Prob. 11SAQCh. 9 - Prob. 12SAQCh. 9 - Use formal charge to choose the best Lewis...Ch. 9 - Use bond energies to determine Hrxnfor this...Ch. 9 - Prob. 15SAQCh. 9 - Prob. 1ECh. 9 - Prob. 2ECh. 9 - Prob. 3ECh. 9 - Prob. 4ECh. 9 - Prob. 5ECh. 9 - Prob. 6ECh. 9 - Prob. 7ECh. 9 - Prob. 8ECh. 9 - Explain the trend in the lattice energies of the...Ch. 9 - Prob. 10ECh. 9 - The lattice enerqy of CsF is -744 kJ/mol, whereas...Ch. 9 - Prob. 12ECh. 9 - Prob. 13ECh. 9 - Prob. 14ECh. 9 - Prob. 15ECh. 9 - Prob. 16ECh. 9 - Prob. 17ECh. 9 - Prob. 18ECh. 9 - Draw the Lewis structure for CO with an arrow...Ch. 9 - Prob. 20ECh. 9 - Prob. 21ECh. 9 - Prob. 22ECh. 9 - Prob. 23ECh. 9 -
24. Write the Lewis structure that obeys the...Ch. 9 - Prob. 25ECh. 9 - Use formal charge to determine which of the two...Ch. 9 - Prob. 27ECh. 9 - Prob. 28ECh. 9 - Prob. 29ECh. 9 - Prob. 30ECh. 9 - Prob. 31ECh. 9 - What are the formal charges of the atoms shown in...Ch. 9 - Write the Lewis structure for each molecule. a....Ch. 9 - Prob. 34ECh. 9 - Prob. 35ECh. 9 - Prob. 36ECh. 9 - Prob. 37ECh. 9 - Prob. 38ECh. 9 - Consider these three compounds: HCCH, H2CCH2...Ch. 9 - Prob. 40ECh. 9 - Prob. 41ECh. 9 - Prob. 42ECh. 9 - Prob. 43ECh. 9 - Prob. 44ECh. 9 - Prob. 45ECh. 9 - Prob. 46ECh. 9 - Prob. 47ECh. 9 - Amino acids are the building blocks of proteins....Ch. 9 - Prob. 49ECh. 9 - Prob. 50ECh. 9 - Prob. 51ECh. 9 - Prob. 52ECh. 9 - Prob. 53ECh. 9 - Prob. 54ECh. 9 - Prob. 55ECh. 9 - Prob. 56ECh. 9 - Prob. 57ECh. 9 - Prob. 58ECh. 9 - Prob. 59ECh. 9 - Prob. 60ECh. 9 - Prob. 61ECh. 9 - Prob. 62ECh. 9 - Prob. 63ECh. 9 - Calculate Hrxn for the combustion of octane...Ch. 9 - 65. Draw the Lewis structure for each compound.
a....Ch. 9 - Prob. 66ECh. 9 - Prob. 67ECh. 9 - Prob. 68ECh. 9 - Prob. 69ECh. 9 - Prob. 70ECh. 9 - Prob. 71ECh. 9 - Prob. 72ECh. 9 - Prob. 73ECh. 9 - Prob. 74ECh. 9 - Prob. 75ECh. 9 - Prob. 76ECh. 9 - Prob. 77ECh. 9 - Prob. 78ECh. 9 - Prob. 79ECh. 9 - Prob. 80ECh. 9 - Prob. 81ECh. 9 - Prob. 82ECh. 9 - Prob. 83E
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- Lewis structures can be used to understand why some molecules react in certain ways. Write the Lewis structures for the reactants and products in the reactions described below. a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide. b. Boron trihydride accepts a pair of electrons from ammonia, forming BH3NH3. Give a possible explanation for why these two reactions occur.arrow_forwardWhat is the connection between bond order, bond length, and bond energy? Use ethane (C2H6), ethylene (C2H4), and acetylene (C2H2) as examples.arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward
- An important observation supporting the concept of resonance in the localized electron model was that there are only three different structures of dichlorobenzene (C6H4C10). How does this fact support the concept of resonance (see Exercise 89)?arrow_forwardDinitrogen monoxide, N2O, can decompose to nitrogen and oxygen gas: 2 N2O(g) 2 N2(g) + O2(g) Use bond dissociation enthalpies to estimate the enthalpy change for this reaction.arrow_forwardUse the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔHrxn° for the equation C2H4 (g) + HBr (g) --> C2H5Br (g) Average molar bond enthalpies. (?bond)(Hbond) Bond ??⋅???−1kJ⋅mol−1 Bond ??⋅???−1kJ⋅mol−1 O−HO−H 464464 C≡NC≡N 890890 O−OO−O 142142 N−HN−H 390390 C−OC−O 351351 N−NN−N 159159 O=OO=O 502502 N=NN=N 418418 C=OC=O 730730 N≡NN≡N 945945 C−CC−C 347347 F−FF−F 155155 C=CC=C 615615 Cl−ClCl−Cl 243243 C≡CC≡C 811811 Br−BrBr−Br 192192 C−HC−H 414414 H−HH−H 435435 C−FC−F 439439 H−FH−F 565565 C−ClC−Cl 331331 H−ClH−Cl 431431 C−BrC−Br 276276 H−BrH−Br 368368 C−NC−N 293293 H−SH−S 364364 C=NC=N 615615 S−SS−S 225225arrow_forward
- Use average bond energies to estimate the enthalpy changes of the following reaction? 2HF-->H2 + F2 a. -466kJ b. +38.6kJ c, -413kJ d. -93kJarrow_forwardThe molecule 2-butene, C4H8, can undergo a geometric change called cis-trans isomerization. (Figure 1) Such transformations can be induced by light and are the key to human vision. Rotation about the C=C bond, which breaks the π bond, is required for the isomerization. The average bond energy (enthalpy) for a C=C double bond is 614 kJ/mol and that of a C−C single bond is 348 kJ/mol. Estimate the energy needed to break only the π bond of the double bond of 2-butene.Express your answer numerically in joules per molecule.arrow_forwardUse bond energies to calculate the heat of reaction: H4C2+Cl2=H4Cl2C2 = kJarrow_forward
- Based on bond enthalpies, which do you expect to be more reactive? Based on bond enthalpies, which do you expect to be more reactive? oxygen, O2 hydrogen peroxide, H2O2arrow_forwardUse the bond energies provided to estimate ΔH°rxn for the reaction below. CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) Cl-Cl 243 H-Cl 432 C-Cl 339 H-C 413 Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) Cl-Cl 243 H-Cl 432 C-Cl 339 H-C 413 answers: -643 kJ -2624 kJ -460 kJ +572 kJ +3084 kJarrow_forwardUse the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation C2H4 (g) + HBr (g) --> C2H5Br(g) Average molar bond enthalpies. (?bond) Bond ??⋅???−1 Bond ??⋅???−1 O−H 464 C≡N 890 O−O 142 N−H 390 C−O 351 N−N 159 O=O 502 N=N 418 C=O 730 N≡N 945 C−C 347 F−F 155 C=C 615 Cl−Cl 243 C≡C 811 Br−Br 192 C−H 414 H−H 435 C−F 439 H−F 565 C−Cl 331 H−Cl 431 C−Br 276 H−Br 368 C−N 293 H−S 364 C=N 615 S−S 225arrow_forward
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