Calculate the enthalpy of reaction for the equation using the bond energy values given. C₂H4+302 → 2CO2 + 2H₂O Bond Energy Bond Energy Bond Bond Lewis Structures (kJ/mol) (kJ/mol) C-H 413 O-H 463 H 0-0 146 0=0 498 C=C 0=0 C-C 346 C=C 602 H C-O 358 C=O 799 O=c=0; H ΔΗxn = [ ? ] kJ Enter a + or - sign AND the magnitude in your answer. Enter

Calculate the enthalpy of reaction for the equation using the bond energy values given. C₂H4+302 → 2CO2 + 2H₂O Bond Energy Bond Energy Bond Bond Lewis Structures (kJ/mol) (kJ/mol) C-H 413 O-H 463 H 0-0 146 0=0 498 C=C 0=0 C-C 346 C=C 602 H C-O 358 C=O 799 O=c=0; H ΔΗxn = [ ? ] kJ Enter a + or - sign AND the magnitude in your answer. Enter

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

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Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔ⁢Hrxn° for the equation NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)NH3⁢(g)+2⁢O2⁡(g)⟶HNO3⁢(g)+H2O(g) The bonding in the molecules is shown.
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
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 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
Use the data found in Thermodynamic Properties to determine the values for the O-Cl and the O-F bond energies. (heats of formation of OF2 and OCl2 are 24.7 and 80.37 kJ/mol, respectively). Please see https://youtu.be/-OKWJ0LYdNc for assistance. DO-F kJ/mol DO-Cl kJ/mol
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
Given the following thermodynamic data, calculate the lattice energy of LiCl:ΔH°f[LiCl(s)] = -409 kJ/molΔH°sublimation [Li] = 161 kJ/molBond energy [Cl-Cl] = 243 kJ/molIE1 (Li) = 520 kJ/molEA1 (Cl) = -349 kJ/mol -1682 kJ/mol -984 kJ/mol -1560 kJ/mol -862 kJ/mol -1213 kJ/mol
Calculate the enthalpy change for the following reactions using the bond enthalpy given below. (Bond enthalpy/kJ : H−H = 436, C−H = 413, C=O = 799, O=O = 495, O−H = 463) (a) H2(g) + 1⁄2O2(g) → H2O(g) (b) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
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
Use the bond energies provided to estimate the enthalpy for the reaction below 2Br2(l) + C2H2(g) --> C2H2Br4(l) Bond Bond Energy (kJ/mol) Br single bond Br 193 C triple bond C 837 C single bond C 347 C single bond Br 276 C single bond H 414
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