Question

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The equation for the reaction can be shown as:
HH
H-C-0-0-H
+ 30=
0
2
0=C=O
+ 3H-O-H
HH
Bond
Bond energy in
KJ per mole
413
347
C-H
C-C
C-O
C=0
O-H
O=0
358
799
467
495
Use the bond energies to calculate the overall energy change for this
reaction.
Overall energy change = ...

Answer 1

`\large \boxed{\text{-1276 kJ/mol}}`

Step-by-step explanation:

You calculate the energy required to break all the bonds in the reactants.

Then you subtract the energy needed to break all the bonds in the products.

CH₃CH₂OH + 3O₂ ⟶ 2CO₂ + 3H₂O

Bonds: 5C-H 1C-C 1C-O 1O-H 3O=O 4C=O 6O-H

D/kJ·mol⁻¹: 413 347 358 467 495 799 467

`\Delta H = \sum{D_{\text{reactants}}} - \sum{D_{\text{products}}}\\\sum{D_{\text{reactants}}} = 5 * 413 + 1 * 347 + 1 * 358 + 1 * 467 + 3 * 495 = 3237 + 1485\\=\text{4722 kJ}\\\sum{D_{\text{products}}} = 4 * 799 + 6 * 467 =3196 + 2802 = \text{5998 kJ}\\\Delta H = 4722 - 5998= \textbf{-1276 kJ} \\ \text{The overall energy change is $\large \boxed{\textbf{-1276 kJ/mol}}$}.`