H H-C-HQ) + 20=0(0) O=C=0(a) + 2H-O-Hq) Bond enthalpies: C-H = +424 kJ/mol; C==0 = +805...
4. Use the bond enthalpies below and calculate the enthalpy of ethane combustion in kJ / mol. (AH° (H-H) = 436 kJ mol', AH° (C-H) = 435 kJ mol', AH° (0=0) = 498, AH° (CEO) = 732, AH (H-O) = 463] CzH6 (g) + 7/202 (g) - 2002 + 3H20 (g)
Use bond enthalpies (in kJ/mol): C-C 348 C=C 614 C≡C 839 H-H 436 C-H 413 O-H 463 C-O 358 C=O 799 to estimate ΔH for the reaction H2C=CH–CH2–OH (g) = > HC≡C–CH=O(g) + 2 H2(g)
Using the bond enthalpies in
the Average Bond Enthalpies table, determine the approximate
enthalpy (in kJ) for each of the following reactions. (Assume the
average bond enthalpy of the Cl–F bond is 254 kJ/mol.) (a) Cl2(g) +
3 F2(g) → 2 ClF3(g) (b) H2C=CH2(g) + H2(g) → H3CCH3(g) (c) 2
CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g)
ITITIT Average Bond Enthalpies AH bond (kJ/mol) bond AHond (kJ/mol) bond AH bond (kJ/mol) bond bond AH bond (kJ/mol) С-Н...
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347 kJ/mol C=C 620 kJ/mol Substance & delta Hf H2 0 C2H4 52.3 C2H6 -84.7 (a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol (b) Calculate the enthalpy of reaction, using standard enthalpies of formation
Bond Avg Bond Strength (in kJ/mol) C-C 350 C=O (in CO2) 804 O=O (in O2) 498 O-H 464 C-H 415 The table above gives the average bond strength for a variety of chemical bonds. Use these values to calculate the energy change (in kJ) for the combustion of 24.8 grams of propane? If your answer is positive include no sign, if it is negative, include a negative sign. kJ
C-H Bond H3 C-H 422 372 C2H3-H (H3C)2HC-H (H3C)3C-H CR3-H HC=C-H R = alkyl C-H Bond Dissociation Enthalpies in kJ/mol BDE (kJ/mol) C-H Bond BDE (kJ/mol) C-H Bond BDE (kJ/mol) 439 RH, C-H HAC-HC-HAC-H | 422 R2HC-H 414 RHC=HC-RHC-H 372 414 H2C=HC-H 464 RHC=RC-RHC-H 372 405 RHC=HC-H 464 R2C=RC-RHC-H 372 405 RAC-HC-H 464 Ar-H 472 556 RC=C-H 556 Ar-H, C-H Ar = aromatic Ar(H3C)HC-H 376 376 Use the above table to estimate the bond dissociation enthalpy (BDE) of each indicated...
Calculate AH for the following reaction using the given bond dissociation energies. >co,g)+2H,0(g) AH° (kJ/mol) CHg)20,g) Bond 142 О-О Н-О 459 С-Н 411 799 O O 498 С-О 358 Number ΔΗ. kJ/ mol This reaction is endothermic exothermic
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the CI-F bond is 254 kJ/mol.) (a) C12(g) + 3 F2(9) ► 2 CIF3(9) -817 kJ (b) H_C=CHCH2(g) + H2(9) ► H,CCH, CH3(9) 476x kJ (c) CHz(C=O)CH3(g) + 402(9) ► 300,(9) + 3 H20(9) 127 X kJ Supporting Materials Periodic Table 1 Supplemental Data Constants and Factors Additional Materials eBook
Use the bond energies provided to estimate AH'rxn for the reaction below. H :C=o: + 2H-H - → H-C-0-H - I O-119 kJ +137 kJ -555 bed -252 kJ +2731
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9) Given the bond enthalpies Cl-Cl (243), C-CI (339), H-CI (431),C-H (414)all in kJ/mol, estimate AE for the following reaction: CH4(g)+ Cl2(g)-CH3Cl(g)+ HCl(g) A)-1427 k) B) -113 kJ C) -30 kJ D)-356 kJ E) 301 kJ