Answer
See the explanation
Work Step by Step
To estimate the change in energy (ΔE) for each of the given reactions, we can use the bond energy values provided in Table 3-3.
a. $CH_{2}-CH_{2}+HCN\rightarrow HOH-C-N=N$
The bond energies involved in this reaction are:
- C-C bond: 347 kJ/mol
- C-H bond: 413 kJ/mol
- C≡N bond: 887 kJ/mol
- O-H bond: 463 kJ/mol
- N=N bond: 945 kJ/mol
The change in energy (ΔE) for this reaction can be calculated as:
ΔE = (887 + 945) - (347 + 413 + 463) = 609 kJ/mol
b. $HOCH_{2}CH_{2}CN\rightarrow \underset {H}{C}=C^{H}+H_{2}O$
The bond energies involved in this reaction are:
- C-O bond: 358 kJ/mol
- C-C bond: 347 kJ/mol
- C-H bond: 413 kJ/mol
- C≡N bond: 887 kJ/mol
- C=C bond: 611 kJ/mol
- O-H bond: 463 kJ/mol
The change in energy (ΔE) for this reaction can be calculated as:
ΔE = (611 + 463) - (358 + 347 + 413 + 887) = 69 kJ/mol
c. $4CH_{2}=CHCH_{3}+6NO\frac {700^{\circ }C}{Az}\\ 4CH_{2}=CHCN+6H_{2}O+N_{2}$
The bond energies involved in this reaction are:
- C=C bond: 611 kJ/mol
- C-H bond: 413 kJ/mol
- C≡N bond: 887 kJ/mol
- N=O bond: 630 kJ/mol
The change in energy (ΔE) for this reaction can be calculated as:
ΔE = (4 × 887 + 6 × 630) - (4 × 611 + 4 × 3 × 413) = 1,320 kJ/mol
