(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

The overall activation energy E is 60 kcal/mol.

Reaction steps are:

CH3CHO --> .5CH3CO + .5CH3 + .5H2 E1 = 80 kcal/mol

CH3CO --> CH3 + CO E2 = ?

CH3 + CH3CHO --> CH4 + CH3CO E3 = 10 kcal/mol

CH3 + CH3CO --> minor products E4 = 5 kcal/mol

Estimate E2.

2. Relevant equations

Arrhenius equation k = A exp (-E/RT)

3. The attempt at a solution

Does E1 + E2 + E3 + E4 = E? If so, then E2 = -35 kcal/mol. If this is the case, what does negative activation energy mean (physically)?

Do I need to use the Arrhenius equation and/or d[M]/dt expressions to solve this problem. Since E1 >> E3 and E4, are there any assumptions I can make?

I feel like I'm missing something here.

Thanks!

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# Homework Help: Reaction steps and Activation Energies

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