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goldsomecriss Aug 12th 2017 07:42 PM

rate law and mechanism
 
Rate Laws and Mechanisms?

The reaction and rate law for the gas-phase decomposition of dinitrogen pentaoxide are*
2N2O5(g) → 4NO2(g) + O2(g)*
rate = k[N2O5]*
Which of the following are valid mechanisms for the reaction?*

1.*
N2O5 ⇌ NO3(g) + NO2(g) [fast]*
NO2(g) + N2O5(g) → 3NO2(g) + O(g) [slow]*
NO3(g) + O(g) → NO2(g) + O2(g) [fast]*

2.*
one step collision*

3.*
2[N2O5(g) → NO3(g) + NO2(g)] [slow]*
2[NO3(g) → NO2(g) + O(g)] [fast]*
2O(g) → O2(g) [fast]*

4.*
2N2O5(g) → N4O10(g) [slow]*
N4O10(g) → 4NO2(g) + O2(g) [fast]*

5.*
2N2O5(g) ⇌ 2NO2(g) + N2O3(g) + 3O(g) [fast]*
N2O3(g) + O(g) → 2NO2(g) [slow]*
2O(g) → O2(g) [fast]



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adianadiadi Oct 24th 2017 09:27 PM

It seems the rate depends on the concentration of only nitrogen pentaoxide.


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