On reactant side we have:
1 C≡C bond
2 C-H bond
2 H-I bond
On product side we have:
4 C-H bond
1 C-C bond
2 C-I bond
Use:
Delta H = BE(reactant) - BE(product)
=1*BE(C≡C) + 2*BE(C-H) + 2*BE(H-I) - 4*BE(C-H) - 1*BE(C-C) - 2*BE(C-I)
=1*839 + 2*413 + 2*299 - 4*413 - 1*348 - 2*240
= -217 KJ
Answer: -217 KJ
13. (12 pts) Using the following bond dissociation energies, estimate the enthalpy of the reaction for...
Using the table of average bond energies below, the AH for the reaction is kJ. нн H-CEC-H(g) 2HI (g) I-CC-I(g) нн Bond: CECC-C H-1 C-IC-H D (kJ/mol): 839 348 299 240 413 -63 -160 +160 +63 -217 B. Are the following statements true or false? Consider the hypothetical molecule B A Drag the appropriate statements to their respective bins. Help Reset If resonance was important, the molecule would have identical A bond lengths. This molecule cannot exist true false
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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
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
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...
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
Part A. Find the average enthalpy of the PF bond in PF5(g) from the following standard molar enthalpies of formation (in kJ/mol): PF5(g) (–1595), P(g) (315), F(g) (79). Part B. Using the bond energies from the table below estimate AH for the following reaction C2H2(g) + H2(g) → C2H4(g) Bond Bond energy [kJ/mol] [C-H 413 H-H 436 |C-C 348 C=C 614 csc 839
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....
Please show work! I've tried this problem a few times, but seem to be going wrong somewhere. The answer should be 366 kJ/mol, but I do not understand how to arrive at that solution. Thank you! a.) AHxn for the reaction below was determined using bond dissociation energies (BDEs) to be -57 kJ Using the table of BDE below, find the bond energy for H-Br c-C НН НН H-C-C-Br НН + H-Br Bond C-C с-с C-H C-Br H-Br Bond Enthalpy...
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