Use the table of standard bond energies given below to calculate the energy of reaction for the following chemical reaction.HO C= OH-H+O CO HStandard Single Bond Energies(in kJ/mol)HCOFCIH432411346459358142565155485190428327218249240Standard Multiple Bond EnergiesC=CC=00=0CEC602799494835AnswerEnter your answer hereBackLeave blankNextCOF C

One C=O and one H-H bonds are broken.Using the reference table, the bond enthalpy of C=O and H-H are…

Answered: Use the table of standard bond energies…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.21QE

See similar textbooks

Similar questions

Use 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 225
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. C2H4(g) + H2O2(g) --> CH2OHCH2OH(g) ΔHreaction = ?
Estimate the enthalpy of the reaction below using the following enthalpies (kJ/mol): NN single bond=160 NN double bond =418, triple bond = 941 HH bond= 432 NH bond =391. N2+ 3H2 -> 2NH3 A. -109 kJ/mol B. +1455 kJ/mol C. -890 kJ/mol D. -632 kJ/mol
Use 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 225225
Using the table of bond energies below, estimate the enthalpy change (kJ) for the following reaction: CH4+2O2⟶CO2+2H2O Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891 Cl-Cl 243
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
Using the table of bond energies above, estimate the enthalpy change (kJ) for the following reaction: 2NCl3(g)⟶N2(g)+3Cl2(g) Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891 Cl-Cl 243 S-Cl 250 S=O 535 S-S 215 S-O 364 S-H 339
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)
C(s) → C(g), ΔH = +715 kJmol-1 Cl2(g) → 2Cl(g), ΔH = +242 kJmol-1 C(s) + 2Cl2(g) → CCl4(g), ΔH = -135.5 kJmol-1 Calculate the average bond dissociation enthalpy of a C-Cl bond.
Estimate the carbon–fluorine bond energy given that the C-C bond energy is 347 kJ/mol, the C=C bond energy is 614 kJ/mol, and the F-F bond energy is 154 kJ/mol. Delta H = -549 kJ
How many grams of CO2 are produced when C3H8 is combusted in oxygen and 507.0 kJ of heat are released? Estimate ΔHrxn using bond enthalpies from the table above in order to solve this problem. Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891
Use bond energies from the table to estimate ΔrH for the following reaction. C2H2(g)+H2(g)→C2H4(g) ΔrH=? Express the answer in kJ/mol to three significant figures.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS