Here ∆H° (C-C) not given so that value is taken from Google. Please check this value with your text book value.
4. Use the bond enthalpies below and calculate the enthalpy of ethane combustion in kJ / mol. (AH° (H-H) = 436 kJ m...
Calculate the enthalpy for the reaction below using the following bond dissociation energies. • H-H 436 kJ/mol O-H 460 kJ/mol 0-0 180 kJ/mol • 0=0 498 kJ/mol H -774 kJ/mol -654 kJ/mol 654 kJ/mol 774 kJ/mol
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)
16) (10 pts.) Using the table of average bond energies below, what is AH for the reaction? HaC-O-H (g) → CEO(g) + 2H2(g) 413 Bond: Enthalpy (kJ/mol):358 1072 436 463 799
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...
Estimate AHrxn for the below chemical reaction using the provided bond enthalpies. The Lewis structures hydrogen peroxide (H2O2) is shown below. 2 H2O2 (g) → 2 H20 (g) + O2 (g) Bond Bond Enthalpy (kJ/mol) 0-0 O=0 495 H-O 463 Η-Η 436 146 : 0:1
Balance the equation for the complete combustion of ethane: C2H6 (g) + O2 (g) ⟶⟶CO2 (g) + H2O (g). Calculate ΔΔHofor the reaction per mole of ethane using the given bond dissociation energies. →CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
8. Ethanol is a common biofuel additive for gasoline. Estimate AH (kJ mol) for the combustion reaction of ethanol. Potentially useful bond energies are: H-H = 436 kJ/mol, O=0 = 499 kJ/mol, O-H 463 kl/mol, C=O = 799 kl/mol, C-O 358 kJ/mol, C-H= 411 kJ/mol, C-C = 346 kJ/mol a) -6000 b) - 1601 c) -1250 d) o e) + 4700
The enthalpy change for the following reaction is 95.4 kJ. Using bond energies, estimate the N-H bond energy in N2H4(g). N2(g) + 2H2(g) N2H4(g) kJ/mol The enthalpy change for the following reaction is -92.2 kJ. Using bond energies, estimate the H-H bond energy in H2(g). 2NH3(g) N2(g) + 3H2(g) kJ/mol D Single Bonds Multiple Bonds C N O F Si P S a Br 1 H 436 413 391 463 565 318 322 347 C 413 346 305 358 485...
Use bond energies to estimate the enthalpy of formation of HBr(g). BE(H–H) = 436 kJ/mol BE(Br–Br) = 192 kJ/mol BE(H–Br) = 366 kJ/mol A –52 kJ/mol B +262 kJ/mol C +104 kJ/mol D +52 kJ/mol E –104 kJ/mol
a. b. For b is this table below: Bond Bond Energy, D (kJ/mol) C=0 1072 C1-C1 242 C-CI 339 C=0 732 Using the values of bond energy from the table above, estimate the enthalpy change for the following reaction: CO(g) + Cl2(9)—>COC12(E) DkJ Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: H2(g) + 12(8)—2HI(g) kJ Submit Answer Retry Entire Group 6 more group attempts remaining Single Bonds H C N O F Si P...