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

Question

To understand how elementary steps make up a mechanism and how 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 NO_2(g) + CO(g) rightarrow NO(g) + CO_2(g) does not solve a collision between an NO_2 molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: NO_2(g) + NO_2(g) rightarrow NO_2(g) + NO(g) NO_2(g) + CO(g) rightarrow CO_2(g) + NO_2(g) Each individual step is called an elementary step. Together these elementary steps are called the reaction mechanism. Overall the resulting reaction is NO_2(g) + CO(g) rightarrow NO(g) + CO_2(g) What is the rate law for step 1 of this reaction? Express your answer in standard mastering chemistry reaction. For example, if the rate law is k[A][C]^3 type is What is the rate law for step 2 of this reaction? Express your answer in standard mastering chemistry reaction. For example, if the rate law is k[A][C]^3 type is

Explanation / Answer

What is rate law for step 1 of this reaction

. Step (1): NO2 + NO2-------à NO3 + NO

Rate (1)= k1 [NO2]^ 2

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Step (2): NO3 + CO -----àNO2 +CO2

Rate (2) = k2 [NO3][CO]

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Overall Reaction: 2 NO2 + CO---à NO + CO2

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