Answer
The estimated change in energy (ΔE) for the given gas phase reaction is 303 kJ/mol.
Work Step by Step
To estimate the change in energy (ΔE) for the given gas phase reaction using bond energy values, we need to calculate the total bond energies of the reactants and products, and then find the difference.
The reaction is:
$C_{2}H_{4} + H_{2}O_{2} \rightarrow CH_{2}OHCH_{2}OH$
The bonds broken are:
1 C=C bond energy: 614 kJ/mol
1 O-O bond energy: 146 kJ/mol
The bonds formed are:
1 C-C bonds (347 kJ/mol)
2 C-O bonds (2 × 358 = 716 kJ/mol)
ΔE = 614 + 146-(347+716)= -303 kJ/mol
Therefore, the estimated change in energy (ΔE) for the given gas phase reaction is $303$ kJ/mol.
