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50./
This question is about calculating bond energies of the reaction below.
2H2 + O2 --> 2 H2O
Bond Energy = Broken - Formed
It takes positive energy to break bonds, but when bonds form, energy is released, so I assumed that O-H bond energies must be converted to negative values. But the answer did not change signs for bond formation. Why??
53.
O3 <-- --> O2 + O (Fast)
O3 + O <-- --> 2 O2 (slow)
Why is it that the rate law is
Rate = k[O3][O]?
Isn't O an intermediate so it doesn't count??? Or am I just confused??
This question is about calculating bond energies of the reaction below.
2H2 + O2 --> 2 H2O
Bond Energy = Broken - Formed
It takes positive energy to break bonds, but when bonds form, energy is released, so I assumed that O-H bond energies must be converted to negative values. But the answer did not change signs for bond formation. Why??
53.
O3 <-- --> O2 + O (Fast)
O3 + O <-- --> 2 O2 (slow)
Why is it that the rate law is
Rate = k[O3][O]?
Isn't O an intermediate so it doesn't count??? Or am I just confused??
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