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Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Rate = - Δ[Α] At = k[A][B]² -2 An experiment is carried out where [A] = 1.0 × 10-² M, [B]₁ = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10 M. -3 a. Calculate the value of k for this reaction. L² mol 2S-1 k = 1.21 b. Calculate the half-life for this experiment. Half-life = 5.7 S c. Calculate the concentration of A after 11.0 seconds. Concentration = 2.6x10^-3 M d. Calculate the concentration of C after 11 seconds. Concentration = 2.0 M

Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Rate = - Δ[Α] At = k[A][B]² -2 An experiment is carried out where [A] = 1.0 × 10-² M, [B]₁ = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10 M. -3 a. Calculate the value of k for this reaction. L² mol 2S-1 k = 1.21 b. Calculate the half-life for this experiment. Half-life = 5.7 S c. Calculate the concentration of A after 11.0 seconds. Concentration = 2.6x10^-3 M d. Calculate the concentration of C after 11 seconds. Concentration = 2.0 M

Chemistry
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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Consider the hypothetical reaction A + B + 2C 2D + 3E where the rate law is Rate = Δ[Α] At = k[A][B]² An experiment is carried out where [A]o seconds, the concentration of A is 3.8 x 10 Submit Answer -2 1.0 × 10-² M, [B] = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0 -3 M. = a. Calculate the value of k for this reaction. -2 L² mol s k = 1.21 b. Calculate the half-life for this experiment. Half-life = 5.7 S c. Calculate the concentration of A after 11.0 seconds. Concentration = 2.6x10^-3 M d. Calculate the concentration of C after 11 seconds. Concentration = 2.0 M An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Retry Entire Group -1 2 more group attempts remaining Previous Next
Transcribed Image Text:Consider the hypothetical reaction A + B + 2C 2D + 3E where the rate law is Rate = Δ[Α] At = k[A][B]² An experiment is carried out where [A]o seconds, the concentration of A is 3.8 x 10 Submit Answer -2 1.0 × 10-² M, [B] = 3.0 M, and [C] = 2.0 M. The reaction is started, and after 8.0 -3 M. = a. Calculate the value of k for this reaction. -2 L² mol s k = 1.21 b. Calculate the half-life for this experiment. Half-life = 5.7 S c. Calculate the concentration of A after 11.0 seconds. Concentration = 2.6x10^-3 M d. Calculate the concentration of C after 11 seconds. Concentration = 2.0 M An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Retry Entire Group -1 2 more group attempts remaining Previous Next
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