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A proposed mechanism is given for the reaction O3(g) + O(g) --> 2 O2(g). Determine the...

A proposed mechanism is given for the reaction O3(g) + O(g) --> 2 O2(g). Determine the rate law for this proposed mechanism, showing all work. Also identigy the intermeditate in this mechanism. (this isn't needed, but can you explain briefly how to decipher the intermediate for future reference please?)

Step 1: O3 + NO --> NO2 + O2 (slow)

Step 2: NO2 + O --> NO + O2 (fast)

Rate= __________________________ Intermediate = __________________________

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Answer #2

Given that O3(g) + O(g) ----------> 2 O2 (g)         ------- Eq(1)

Mechanism:

Step 1: O3 + NO --> NO2 + O2 (slow)

Step 2: NO2 + O --> NO + O2   (fast)

Then,

Slowest step is always the rate determining step of the reaction.

Therefore,

rate = k [O3] [NO]

Intermediate:

The species other than reactants and products present in the reaction mechanism are called intermediates.

As per the Eq(1),

O3 , O = reactants

O2 = product

Therefore,

NO2, NO are intermediates.

answered by: anonymous
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