Question

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

Step 2: NO₂ + O --> NO + O₂

Rate= __________________________ Intermediate = __________________________

Answer 1

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

Mechanism:

Step 1: O₃ + NO --> NO₂ + O₂

Step 2: NO₂ + O --> NO + O₂

Then,

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

But, no information given about slowest step.

So,

rate = k [O₃] [O]

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