Using average bond enthalpy values estimate the heat (kJ/mol) given off in the following gas phase reaction.
2CH2=CHCH3 + 2NH3 + 3O2 --> 2CH2=CHCN + 6H2O
First I calculated the:
Number of Bonds/type of bonds being formed:
2 C=N
12 H-O
Number of Bonds/ type of bonds being broken:
6 C-H
6 N-H
3 O=O
Avg Bond enthalpies (in kJ/mol)
C=N = 866
H-O = 467
C-H = 416
N-H = 391
O=O = 498
What I did was add the enthalpies of the bonds form and add the enthalpies broken and subtract.
So this is what i did:
Bonds formed = 2x866 + 12x467 = 7336
Bonds broken = 6x416 + 6x391 + 3x498 = 6336
subtracted = 1000kJ/mol
But when plugging it in as my answer for my online hw, i got an incorrect answer. can anyone guide to the direction that was overlooked?