The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results: Experiment[HBr(g)] (M)[O2(g)] (M)Rate (M/s) 10.005320.005320.23020.005320.01060.45830.01060.005320.45840.01060.01060.912(a) What is the rate law for this reaction?Rate = k [HBr(g)] [O2(g)]Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2Rate = k [HBr(g)]2 [O2(g)]2Rate = k [HBr(g)] [O2(g)]3Rate = k [HBr(g)]4 [O2(g)](b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of HBr(g) is 0.00533 M and that of O2(g) is 0.0145 M if the temperature is the same as that used to obtain the data shown above? M/s

We have to predict the rate law , rate constant , and rate at certain concentration.

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The reaction 4 HBr(g) + O₂(g) 2 H₂O(g) + 2 Br₂(g) was studied at a certain temperature with the following results:

Experiment	[HBr(g)] (M)	[O₂(g)] (M)	Rate (M/s)


1	0.00532	0.00532	0.230
2	0.00532	0.0106	0.458
3	0.0106	0.00532	0.458
4	0.0106	0.0106	0.912

(a) What is the rate law for this reaction?

Rate = k [HBr(g)] [O₂(g)]Rate = k [HBr(g)]² [O₂(g)] Rate = k [HBr(g)] [O₂(g)]²Rate = k [HBr(g)]² [O₂(g)]²Rate = k [HBr(g)] [O₂(g)]³Rate = k [HBr(g)]⁴ [O₂(g)]

(b) What is the value of the rate constant?

(c) What is the reaction rate when the concentration of HBr(g) is 0.00533 M and that of O₂(g) is 0.0145 M if the temperature is the same as that used to obtain the data shown above?

M/s

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