Problem: The mechanism for the reaction described byNO2(g) + CO(g) → CO2(g) + NO (g)is suggested to be(1) 2NO2(g) →(k1) NO3(g) + NO (g) (slow)(2) NO3(g) +CO(g) →(k2) NO2(g) + CO2(g) (fast) Assuming that [NO3] is governed by steady-state conditions, derive the rate law for the production of CO2(g) and enter it in the space below.

FREE Expert Solution

We are being asked to write a rate law for the reaction using the provided mechanism.

Rate law is a mathematical equation that links the rate of a chemical reaction with the concentrations of its reactants.

Rate law is written using the slow step of the reaction (also called the rate-determining step)


Recall that the rate law only focuses on the reactant concentrations and has a general form of:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders


Get the overall reaction: 

Cancel the intermediate species. 


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Problem Details

The mechanism for the reaction described by

NO2(g) + CO(g) → CO2(g) + NO (g)

is suggested to be

(1) 2NO2(g) →(k1) NO3(g) + NO (g) (slow)

(2) NO3(g) +CO(g) →(k2) NO2(g) + CO2(g) (fast) 

Assuming that [NO3] is governed by steady-state conditions, derive the rate law for the production of CO2(g) and enter it in the space below.

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