(a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [0₂(g)]² [NO(g)]² O Rate = k [0₂(g)] [NO(g)]³ O Rate = k [0₂(9)]* [NO(g)] (b) What is the value of the rate constant? Experiment M/S 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature the same as that used to obtain the data shown above?
(a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [0₂(g)]² [NO(g)]² O Rate = k [0₂(g)] [NO(g)]³ O Rate = k [0₂(9)]* [NO(g)] (b) What is the value of the rate constant? Experiment M/S 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature the same as that used to obtain the data shown above?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results:
(a) What is the rate law for this reaction?
O Rate = k [0₂(g)] [NO(g)]
O Rate = k [0₂(g)]² [NO(g)]
O Rate = k [0₂(g)] [NO(g)]²
O Rate = k [O₂(g)]² [NO(g)]²2
O Rate = k [O₂(g)] [NO(g)]³
O Rate = k [0₂(g)]4 [NO(g)]
(b) What is the value of the rate constant?
Experiment
M/s
1
2
3
4
[0₂(g)] (M)
0.0231
0.0231
0.0462
0.0462
[NO(g)] (M)
0.0231
0.0462
0.0231
0.0462
Rate (M/s)
0.112
0.448
0.224
0.896
(c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2F98d59923-63c5-403a-b62b-9d7866b976cb%2Fgoqsp1_processed.png&w=3840&q=75)
Transcribed Image Text:The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results:
(a) What is the rate law for this reaction?
O Rate = k [0₂(g)] [NO(g)]
O Rate = k [0₂(g)]² [NO(g)]
O Rate = k [0₂(g)] [NO(g)]²
O Rate = k [O₂(g)]² [NO(g)]²2
O Rate = k [O₂(g)] [NO(g)]³
O Rate = k [0₂(g)]4 [NO(g)]
(b) What is the value of the rate constant?
Experiment
M/s
1
2
3
4
[0₂(g)] (M)
0.0231
0.0231
0.0462
0.0462
[NO(g)] (M)
0.0231
0.0462
0.0231
0.0462
Rate (M/s)
0.112
0.448
0.224
0.896
(c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?
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