To understand how elementary steps make up a mechanism and hoe the rate law for

Question

To understand how elementary steps make up a mechanism and hoe the rate law for an elementary step can be determined. Very often a reaction does not tell us the whole story. For instance, the reaction does not involve a collision between an NO_2 molecule and a CO molecule. In reality, this reaction occurs in two steps: Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. Overall, the resulting reaction is: Notice that in the elementary steps N_2O_4 appears both as a product and then as a reactant; therefore it cancels out of the final chemical equation.

Explanation / Answer

Part C. Rate law for the first reaction,

rate = k1[NO2]^2

where, k1 is the rate constant

Part D. Rate law for the second reaction would be,

rate = k2[N2O4][CO]

where, k2 is the rate constant

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