Answer
The estimated change in energy (ΔE) for the given reaction is -75 kJ/mol.
Work Step by Step
To estimate the change in energy (ΔE) for the given reaction using tabulated bond energies, we need to calculate the difference between the total bond energies of the reactants and the total bond energies of the products.
The reaction is:
$CH_{3}OH(g) + C\equiv O(g) \rightarrow CH_{3}C-OH(l)$
Step 1: Calculate the total bond energies broken:
3 C-H bond energy = 3x413 kJ/mol
1 O-H bond energy = 463 kJ/mol
1 C≡O bond energy = 1072 kJ/mol
1 C-O: 358
Total bond energies broken = (3 × 413) + 463 + 1072+358 = 3132 kJ/mol
Step 2: Calculate the total bond energies formed:
3 C-H bond energy = 3x413 kJ/mol
1 C-O bond energy = 358 kJ/mol
1 C=O bond energy = 799 kJ/mol
1 C-C bond energy = 348
1 O-H bond energy = 463 kJ/mol
Total bond energies formed = (3 × 413) + 358 + 799+348+463 = 3207 kJ/mol
Step 3: Calculate the change in energy (ΔE) for the reaction.
ΔE = Total bond energy broken - Total bond energy formed
ΔE = 3132 kJ/mol - 3207 kJ/mol = -75 kJ/mol
Therefore, the estimated change in energy (ΔE) for the given reaction is -75 kJ/mol.
