Table 7.1 Average Bond Dissociation Energies Bond Dissociation Bond Dissociation Bond Dissociation Energy kcal/mol (kJ/mol) Energy kcal/mol (kJ/mol) Energy Bond Bond Bond kcal/mol (kJ/mol) C-H 99 (413) N-H 93 (391) C=C 147 (614) C C 83 (347) N-N 38 (160) C=C 201 (839) C-N 73 (305) N-CI 48 (200) C=0* 178 (745) C-0 86 (358) N-0 48 (201) 119 (498) 0=0 C- CI 81 (339) H-H 103 (432) N=0 145 (607) CI-CI 58 (243) 0-H 112 (467) 0=N 213 (891) H-CI 102 (427) 0-CI 49 (203) N=N 226 (946) *The C=0 bond dissociation energies in CO2 are 191 kcal/mol (799 kJ/mol).

Table 7.1 Average Bond Dissociation Energies Bond Dissociation Bond Dissociation Bond Dissociation Energy kcal/mol (kJ/mol) Energy kcal/mol (kJ/mol) Energy Bond Bond Bond kcal/mol (kJ/mol) C-H 99 (413) N-H 93 (391) C=C 147 (614) C C 83 (347) N-N 38 (160) C=C 201 (839) C-N 73 (305) N-CI 48 (200) C=0* 178 (745) C-0 86 (358) N-0 48 (201) 119 (498) 0=0 C- CI 81 (339) H-H 103 (432) N=0 145 (607) CI-CI 58 (243) 0-H 112 (467) 0=N 213 (891) H-CI 102 (427) 0-CI 49 (203) N=N 226 (946) *The C=0 bond dissociation energies in CO2 are 191 kcal/mol (799 kJ/mol).

Chemistry: An Atoms First Approach

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ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 136IP: In Exercise 89 in Chapter 3, the Lewis structures for benzene (C6H6) were drawn. Using one of the...

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Bond Bond enerygy KJ/Mol H-H 336 C-H 414 C-C 347 C-O 360 O-H 464 O=O 498 C=O 736 C=O IN CO2 799 Ethanol is a possible fuel. Use average bond energies to calculate ΔHrxnΔHrxn for the combustion of ethanol. CH3CH2OH(g) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) Express your answer as an integer.
Calculate ΔHrxn for the following chemical reaction given the listed bond energies. C2H4 + H2 → H6C2 Chemical bond Bond energy (kJ/mol) H-H single bond 450 C-H single bond 400 C-C single bond 350 C=C double bond 600
Bond Bond Energy kJ/molkJ/mol H−H 336 C−H 414 C−C 347 C−O 360 O−H 464 O=O 498 C=O 736 C=O in CO2 799 Ethanol is a possible fuel. Use average bond energies to calculate ΔHrxnΔHrxn for the combustion of ethanol. CH3CH2OH(g) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) Express your answer as an integer.
CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g), ΔH = –434 kJBased on the above reaction, what energy change occurs when 2.2 moles of methane (CH4) reacts? 9.5 × 105 J are released 5.2 × 105 J are absorbed. 4.6 × 105 J are absorbed. 5.6 × 105 J are absorbed. 5.4 × 105 J are absorbed.
Use the bond dissociation energies provided to calculate the detla H (in kilojoules) for the combustion of ethylene gas according to the balanced equation provided: C2H4 (g) + 3 O2 (g) equals 2 CO2 (g) + 2 H2O (g)
The gas hydrazine, N2H4, burns in oxygen like this:NHNHH H(g) + O O (g) N N (g) + 2OHH(g)a Count and list the bonds broken in this reaction.b Count and list the new bonds formed.c Calculate the total energy:i required to break the bondsii released when the new bonds form.(The bond energies in kJ / mole are: N2H 391;N2N 158; NN 945; O2H 464; O5O 498.)d Calculate the energy change in the reaction.e Is the reaction exothermic, or endothermic?f Where is energy transferred from, and to?g Comment on the suitability of hydrazine asa fuel.
Calculate the enthalpy of formation, ∆Hof, for C4H9OH using the following data: C4H9OH (l) + 6 O2 (g) → 5 H2O (g) + 4 CO2 (g) ∆Hrxn = -2676 kJ substance O2 (g) H2O (g) CO2 (g) ∆Hof 0 kJ/mol -242 kJ/mol -394 kJ/mol
Given the reaction: ½ H2 (g) + ½ Cl2 (g) --> HCl (g) ΔH = -92 kJ/mol What is the missing bond energy in kJ/mol? H - H BE = 435 kJ/mol H - Cl BE = 431 kJ/mol Cl - Cl BE = ? kJ/mol? A) 96 B) 335 C) 188 D) 88 E) 243
CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g), ΔH = –434 kJBased on the above reaction, what energy change occurs when 2.2 moles of methane (CH4) reacts?
The combustion of ammonia is : 4NH3(g)+5O2(g)--> 4NO(g)+6H2O(g) DeltaH= -905kJ what is the enthalpy of the formation (kJ/mol) of NH3(g) [Heat of formation data: NO(g)=90.4 kJ/ mol, H2O(g)=-241 kJ/mol]
Fructose, C6H1206(S), consists of 5 C-C single bonds, 7 C-O bonds, 7 C-H bonds, and 5 O-H bonds with average bond energies of 348 kJ/mol, 360 kJ/mol, 412 kJ/mol, and 463 kJ/mol respectively. The bond energy for C=O is 799 kJ/mol and O=O is 498 kJ/mol. The molar mass of fructose is 180.12 g/mol. Estimate the change in enthalpy if 2.56 g of fructose undergoes complete combustion at standard temperature and pressure.
Given the following reactions, what is the overall enthalpy change for the following reaction? NH3(g) + HCl(g) --> NH4Cl(s) Reaction (kJ) N2(g) +3H2(g) --> 2 NH3(g) -92 H2(g) + Cl2(g) --> 2 HCl (g) -185 N2(g) +4 H2(g) +Cl2 -->2NH4Cl(s) -629

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