Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? O Rate = k [NO₂(g)] [03(9)] Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(9)1² O Rate = k [NO₂(g)]² [03(9)]² Rate = k [NO₂(g)] [03(9)]³ Rate = k [NO₂(g)]4 [03(9)] O O (b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [03(9)] = 1.42 M? Rate = 2 NO₂(g) + 03(g) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M? M/s
Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? O Rate = k [NO₂(g)] [03(9)] Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(9)1² O Rate = k [NO₂(g)]² [03(9)]² Rate = k [NO₂(g)] [03(9)]³ Rate = k [NO₂(g)]4 [03(9)] O O (b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [03(9)] = 1.42 M? Rate = 2 NO₂(g) + 03(g) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M? M/s
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![Consider the following reaction:
(a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction?
O Rate = k [NO₂(g)] [03(9)]
Rate = k [NO₂(g)]² [03(9)]
O Rate = k [NO₂(g)] [03(9)]²
O Rate = k [NO₂(g)]² [03(g)]²
Rate = k [NO₂(g)] [03(g)]³
Rate = k [NO₂(g)]4 [03(9)]
(b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [O3(9)] = 1.42 M?
Rate =
2 NO₂(g) + 03(g) → N₂05(9) + O₂(g)
M/s.
Rate =
(c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M?
M/s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2F1d8757a1-4b5a-436f-a4f5-0c7c9c57f4ee%2Fa2bpr0n_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following reaction:
(a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction?
O Rate = k [NO₂(g)] [03(9)]
Rate = k [NO₂(g)]² [03(9)]
O Rate = k [NO₂(g)] [03(9)]²
O Rate = k [NO₂(g)]² [03(g)]²
Rate = k [NO₂(g)] [03(g)]³
Rate = k [NO₂(g)]4 [03(9)]
(b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [O3(9)] = 1.42 M?
Rate =
2 NO₂(g) + 03(g) → N₂05(9) + O₂(g)
M/s.
Rate =
(c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M?
M/s
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