Aproposed mechanism for the oxidation of nitric oxide to nitrogen dioxide is shown below. 2 no (g) ⇄ n2o2 (g) fast, reversible step n2o2 (g) + o2 (g) → 2 no2 (g) slow step what rate law is consistent with this mechanism?

What rate law is consistent with this mechanism?

Rate law is the equation that relates the reaction rate with the concentrations of the reactants and constant parameters.

Nitric oxide is  is a colorless gas with the formula NO. It is free radical and has an unpaired electron. While nitrogen dioxide is the chemical compound with formula NO₂. It is an intermediate in the industrial synthesis of nitric acid.

The mechanism for the oxidation of nitric oxide to nitrogen dioxide is shown below:

⇄ fast, reversible step →

rate = rate of slow step =

Therefore is NOT a reactant or a product. So then we should eliminate it from the rate law.

For equilibrium of ⇄

The conversion of products and  reactants are an example of equilibrium

rate forward = rate backward

So the Equilibrium Constant is:

While for Reversible Step of  ⇄

Forward reaction rates and backward reaction rates will become equal quickly

rate forward = rate backward

Therefore it will be

rate = rate of slow step =

Therefore, rate =

rate =

Grade:    9

Subject:  chemistry

Chapter:  oxidation

Keywords: rate law, nitric oxide, nitrogen dioxide, reversible step, oxidation