Consider the following reaction:4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). 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) If the rate constant for this reaction at a certain temperature is 8860, what is the reaction rate when [HBr(g)] = 0.00558 M and [O2(g)] = 0.00825 M?Rate = _____M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0112 M while the concentration of O2(g) is 0.00825 M?Rate =____M/s

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Answered: Consider the following reaction: 4…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 21QRT: The reaction of CO(g) + NO2(g) is second-order in NO2 and zeroth-order in CO at temperatures less...

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Consider the following reaction:

4 HBr(g) + O₂(g) 2 H₂O(g) + 2 Br₂(g)

(a) The rate law for this reaction is first order in HBr(g) and first order in O₂(g). 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)]²

Rate = k [HBr(g)]² [O₂(g)]²

Rate = k [HBr(g)] [O₂(g)]³

Rate = k [HBr(g)]⁴ [O₂(g)]

(b) If the rate constant for this reaction at a certain temperature is 8860, what is the reaction rate when [HBr(g)] = 0.00558 M and [O₂(g)] = 0.00825 M?

Rate = _____M/s.

(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0112 M while the concentration of O₂(g) is 0.00825 M?

Rate =____M/s

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