Consider the reaction A + 2B = C Part A whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B]. [B] (M) (M) (M/s) 0.20 0.050 2.4x10-3 Trial [A] Rate View Available Hint(s) 0.20 0.100 4.8×10-3 0.40 0.050 9.6x10-3 ΑΣφ 3 rate = Submit Part B Complete previous part(s) Provide Feedback 2.

Consider the reaction A + 2B = C Part A whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B]. [B] (M) (M) (M/s) 0.20 0.050 2.4x10-3 Trial [A] Rate View Available Hint(s) 0.20 0.100 4.8×10-3 0.40 0.050 9.6x10-3 ΑΣφ 3 rate = Submit Part B Complete previous part(s) Provide Feedback 2.

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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What are the units of the rate constant, k, in a second- order equation if rate is measured in mol/(L s) and all concentrations are in mol/L? answer options: s–1 L/(mol*s) L2/(mol2*s) mol2/(L2*s)
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Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.917 0.950 0.252 Trial 2 1.83 0.950 0.504 Trial 3 0.917 1.90 0.504 Trial 4 0.818 0.437 0.103 Rate = k[A]1[B]1
What is the rate constant for the reaction?
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1:18 Sun, 16 June bb. = University of South Australia Dashboard Course Outline Content Academic Integrity Assessment In Grades Ө SP2 2024 Chemistry 100 Dashboard > CHEM 1006 > Online Quizzes > Online quiz 4 Question 4 If the rate law for the reaction Correct Mark 1.00 out 2A + 3B → products of 1.00 Remove flag is first order in A and second order in B, then the rate law is rate = a. k[A][B] b. k[A][B]² c. K[A]²[B]² d. k[A][B] e. k[A]²[B] Extensions Resources Your answer is correct. The correct answer is: k[A][B]² Recordings 16 b *༢ དཱི51% 10 ? Yunseo Kwon = ||| о Sunday, 16 June 2024 1:18 am ACST ←
Explain your reasoning, please. Thank you.
In a particular reaction, BrO3- + 5 Br- + H3O+ → 3 Br2 + 9 H2O , the following table below is completed with the initial concentrations of each reactant and the initial rate for each trial. 1.) Write the rate expression for this reaction. (HINT: rate = -Δ[rcts]/Δt = +Δ[pdcts]/Δt ... ) 2.) Write the rate law for this reaction. (HINT: rate = k [rcts]x ... ) 3.) What is the overall order for this reaction? 4.) What is the rate constant (k) for this reaction? Extra Credit: Calculate the rate of this reaction when [BrO3-] = 0.50 M, [Br-] = 0.25 M, and [H3O+] = 0.35 M.
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