Mechanisms and Molecularity < 7 of 18 > I Review | Constants | Periodic Table Part C Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A]C type k* [A] + [C]^3. > View Available Hint(s) Very often, a reaction does not tell us the whole story. For instance, the reaction Rate = NO2(9) + CO(g)→NO(g) + CO2(g) does not involve a collision between an NO, molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: Submit 1. NO2(9) + NO2(9)→NO3(9) + NO(g) 2. NO3(g) + CO(g)→CO2(9) + NO2(9) Part D Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is kA||C type k* [A] * [C]^3. Overall, the resulting reaction is > View Available Hint(s) NO2(9) + CO(9)-→NO(g) + CO2(g) Rate

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Mechanisms and Molecularity
7 of 18
I Review | Constants | Periodic Table
Part C
Learning Goal:
To understand how elementary steps make up a
mechanism and how the rate law for an elementary
step can be determined.
What is the rate law for step 1 of this reaction?
Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C type k* [A] * [C]^3.
» View Available Hint(s)
Very often, a reaction does not tell us the whole story.
For instance, the reaction
NO2(g) + CO(g)→NO(g) + CO2(9)
Rate
does not involve a collision between an NO2
molecule and a CO molecule. Based on experimental
data at moderate temperatures, this reaction is
thought to occur in the following two steps:
Submit
1. NO2(9) +NO2(9)→NO3(g) + NO(g)
2. NO3(9) + CO(g)→CO2(g) +NO2(g)
Part D
Each individual step is called an elementary step.
Together, these elementary steps are called the
reaction mechanism.
What is the rate law for step 2 of this reaction?
Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k* [A] * [C]^3.
Overall, the resulting reaction is
• View Available Hint(s)
NO2(g) + CO(g)→NO(g)+ CO2(9)
Rate =
Notice that in the elementary steps NO3 appears
Transcribed Image Text:Mechanisms and Molecularity 7 of 18 I Review | Constants | Periodic Table Part C Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C type k* [A] * [C]^3. » View Available Hint(s) Very often, a reaction does not tell us the whole story. For instance, the reaction NO2(g) + CO(g)→NO(g) + CO2(9) Rate does not involve a collision between an NO2 molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: Submit 1. NO2(9) +NO2(9)→NO3(g) + NO(g) 2. NO3(9) + CO(g)→CO2(g) +NO2(g) Part D Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k* [A] * [C]^3. Overall, the resulting reaction is • View Available Hint(s) NO2(g) + CO(g)→NO(g)+ CO2(9) Rate = Notice that in the elementary steps NO3 appears
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