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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)]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 9880, what is the reaction rate when [HBr(g)] = 0.00594 M and [O2(g)] = 0.00819 M? Rate =  M/s. (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0119 M while the concentration of O2(g) is 0.00819 M? Rate =  M/s

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 9880, what is the reaction rate when [HBr(g)] = 0.00594 M and [O2(g)] = 0.00819 M? Rate =  M/s. (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0119 M while the concentration of O2(g) is 0.00819 M? Rate =  M/s

Chemistry: The Molecular Science
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)]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 9880, what is the reaction rate when [HBr(g)] = 0.00594 M and [O2(g)] = 0.00819 M?

Rate =  M/s.



(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0119 M while the concentration of O2(g) is 0.00819 M?

Rate =  M/s

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