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 9920, what is the reaction rate when [HBr(g)] = 0.00467 M and [O2(g)] = 0.00876 M?Rate = M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00934 M while the concentration of O2(g) is 0.00876 M?Rate = M/s

To Solve this problem first we have to write the rate law then according to this rate law we will…

Answered: Consider the following reaction: 4…

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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Question

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 9920, what is the reaction rate when [HBr(g)] = 0.00467 M and [O₂(g)] = 0.00876 M?

Rate = M/s.

(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00934 M while the concentration of O₂(g) is 0.00876 M?

Rate = M/s