Consider the following reaction: (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? Ratek [HBr(g)] [O₂(g)] O Rate = k [HBr(g)]² [O₂(g)] O Rate = k [HBr(g)] [O₂(g)]² O Rate = k [HBr(g)]² [0₂(g)]² O Rate = k [HBr(g)] [O₂(g)]³ O Rate = k [HBr(g)]4 [0₂(g)] (b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.0087 Rate = 4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br2₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M? M/S
Consider the following reaction: (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? Ratek [HBr(g)] [O₂(g)] O Rate = k [HBr(g)]² [O₂(g)] O Rate = k [HBr(g)] [O₂(g)]² O Rate = k [HBr(g)]² [0₂(g)]² O Rate = k [HBr(g)] [O₂(g)]³ O Rate = k [HBr(g)]4 [0₂(g)] (b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.0087 Rate = 4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br2₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M? M/S
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 58GQ: Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of...
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![Consider the following reaction:
(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)]
O Rate = k [HBr(g)]² [O₂(g)]
O Rate = k [HBr(g)] [O₂(g)]²
O Rate = k [HBr(g)]² [0₂(g)]²
O Rate = k [HBr(g)] [O₂(g)]³
O Rate = k [HBr(g)]4 [0₂(g)]
(b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.00876 M?
Rate =
4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br₂(g)
M/s.
Rate =
(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M?
M/S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb30b8e04-1d96-48e3-ae17-9cc7abb41cad%2F6d4d33ca-7501-4cef-a162-791d4b1f93bd%2Fx602xth_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following reaction:
(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)]
O Rate = k [HBr(g)]² [O₂(g)]
O Rate = k [HBr(g)] [O₂(g)]²
O Rate = k [HBr(g)]² [0₂(g)]²
O Rate = k [HBr(g)] [O₂(g)]³
O Rate = k [HBr(g)]4 [0₂(g)]
(b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.00876 M?
Rate =
4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br₂(g)
M/s.
Rate =
(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M?
M/S
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