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Consider this two-step mechanism for a reaction. no2( g) + cl2( g) ¡k1 clno2( g) + cl( g) slow no2( g) + cl( g) ¡k2 clno2( g) fast
a. what is the overall reaction?
b. identify the intermediates in the mechanism.
c. what is the predicted rate law?

Respuesta :

a. Adding the equations gives 2NO2 + Cl2 —> 2ClNO2
b. An intermediate is a chemical formed in the reaction process but is not a reactant or product. The only species that matches this description is Cl
c. Th rate law for any one step reaction is the product of the concentrations of the reactants. Since the slow (rate determining) step is the first one, the expected rate law is k[NO2][Cl2].
pstnonsonjoku

The intermediate Cl occurs on both sides of the reaction equation. The rate law is; k1[NO2] [Cl2]

An elementary reaction is one that occurs in a single reactive encounter while a non - elementary reaction is one that does not occur in a single reactive encounter.

The overall reaction equation for this reaction is;

2NO2(g) + Cl2(g) ------> 2ClNO2(g)

The intermediate in the reaction is Cl. It occur on both sides of the reaction equation hence it cancels out.

The predicted rate law will depend on the slow step which is;

NO2(g)+Cl2(g)⟶k1ClNO2(g)+Cl(g)

Rate = k1[NO2] [Cl2]

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