Given the table of bond energies shown below, what is the estimated enthalpy of reaction of chlorine with methane to produce chloromethane and HCI? Bond Energies (kJ/mol): Н-Н 436 H-F 570 H-CI 432 CI-CI 243 Br-Br 193 I-I 151 CH3-H 438 CH3-CI 351 CH3-Br 293 oa-102 k/mol Ob.+28 k/mol OC.-28 k/mol od. +330 kJ/mol

Given the table of bond energies shown below, what is the estimated enthalpy of reaction of chlorine with methane to produce chloromethane and HCI? Bond Energies (kJ/mol): Н-Н 436 H-F 570 H-CI 432 CI-CI 243 Br-Br 193 I-I 151 CH3-H 438 CH3-CI 351 CH3-Br 293 oa-102 k/mol Ob.+28 k/mol OC.-28 k/mol od. +330 kJ/mol

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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

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

Chapter8: Bonding And Molecular Structure

Section: Chapter Questions

Problem 73GQ: The equation for the combustion of gaseous methanol is 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) (a)...

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Methanol can be made by partial oxidation of methane using O2 in the presence of a catalyst: 2 CH4(g) + O2(g) 2 CH3OH() Use bond dissociation enthalpies to estimate the enthalpy change for this reaction. Compare the value obtained to the value calculated using standard enthalpies of formation.
The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water: OF2(g) + H2O(g) O2(g) + 2 HF(g) rH = 318 kl/mol-rxn Using bond dissociation enthalpies, calculate the bond dissociation enthalpy of the OF bond in OF2.
The equation for the combustion of gaseous methanol is 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) (a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of one mole of gaseous methanol? (b) Compare your answer in part (a) with the value of tHcalculated using enthalpies of formation data.
1,2-Dichloroethylene can be synthesized by adding Cl2 to the carbon-carbon triple bond of acetylene. Using bond dissociation enthalpies, estimate the enthalpy change for this reaction in the gas phase.
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
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
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
Using bond energies from the table below, estimate ΔH for the reaction below. The two oxygens in the reactant are each bound to carbon. One of the hydrogens is bound to carbon.HCOOH(g) ↔ H2(g) + CO2(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 CºC 835 CºN 887 CºO 1072 N=N 418 N=O 607 S=O (in SO2) 532 NºN 942 O2 494 S=O (in SO3) 469
Using the table below where bond energies are in kJ/mol, calculate the enthalpy of the reaction. HC≡C-H + H-I  H2C=CHIC≡C 839 C=C 614H-I 299C-I 240C-H 413 A. 506 B. -931 C. -506 D. -129 E. + 129
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)
Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. C2H4(g) + H2O2(g) --> CH2OHCH2OH(g) ΔHreaction = ?
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 799