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
Use bond energies to estimate the enthalpy of formation of HBr(g). BE(H–H) = 436 kJ/mol BE(Br–Br)...
Estimate the enthalpy of formation of HBr gas.H2(g) + Br2(g) --> 2HBr(g)H-H bond = 436 kJ/molBr-Br bond = 192 kJ/molH-Br bond = 366 kJ/mol
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...
Bond Dissociation Energies (for A-B Bond broken AH, kJ/mol Bond broken → A A4, kJ/mol + B) Bond broken mo H-H CH3CH2CH2-H (CH3)2CH-H (CH3)3C-H 436 423 413 400. H-Br 366 CH3CH2CH2-Br 294 (CH3)2CH-Br 298 (CH3)3C-Br292 Br-Br 193 H-CI 432 CH3CH2CH2-CI 354 (CH3)2CH-CI 355 (CH3)3C-CI 349 CI-CI 243 Alkane halogenation is a two-step reaction, as shown below. Using the table of bond dissociation energies, calculate the enthalpy of each step and the enthalpy of the overall reaction. Step 1: Number CH3CHCH3...
Use the bond enthalpy data given to estimate the enthalpy of reaction for the addition of HBr to acetylene gas, C2H2 to form C2H4Br2 (with the condensed structural formula Br-CH2-CH2-Br ) at 25°C. BE(C-C) = 348 kJ/mol; BE(CC triple bond) = 839 kJ/mol; BE(C-H) = 413 kJ/mol; BE(H-Br) = 366 kJ/mol; BE(C-Br) = 276 kJ/mol -581 kJ/mol -4949 kJ/mol +155 kJ/mol -887 kJ/mol +887 kJ/mol
A Reaction is given: ½Br2(l) --> Br(g) Ho = 112kJ/mol The bond enthalpy of Br-Br is 193 kJ/mol A. Formulate the vaporization process of 1 mol bromine Br2(l). B. Calculate the enthalpy of the vaporization process bromine. Show calculations C. Calculate the energy invested \ emitted by the evaporation of 3.2 gr of bromine. Show calculations. (Explain how you determined whether the energy is invested or emitted in this process). D.A Reaction is given: ½H2(g) + ½Br2(l) --> HBr(g) Ho...
Estimate the enthalpy of formation of HF from the following bond energies: (twenty-five points) H2 (g) + F2 (g) → 2 HF (g) Bond: H-H =432KJ/mol F-F=159 KJ/mol H-F= -565 KJ/mol
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)
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
The enthalpy change for the following reaction is -137 kJ. Using bond energies, estimate the C-C bond energy in C2H6(g) СЭН4(@) + H2(@) — С2Н6(@) kJ/mol Submit Answer Retry Entire Group 7 more group attempts remaining The enthalpy change for the following reaction is -903 kJ. Using bond energies, estimate the N-H bond energy in NH3(g) 4NH3(g)502(g) ANO(g) +6H20(g) kJ/mol Submit Answer Retry Entire Group 7 more group attempts remaining The enthalpy change for the following reaction is -137 kJ....
Using the bond energies from the table below estimate ∆H for the following reaction C2H2(g) + H2(g) → C2H4(g) C-H (413), H-H (436), C-C (348), C=C (614), C≡C (839) A) +165 kJ/mol B) -390. kJ/mol C) +390. kJ/mol D) –124 kJ/mol E) –165 kJ/mol