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Consider the hypothetical reaction A+B+ 2C 2D+3E where the rate law is Rate =- Δ[Α] At k= = k[A][B]² = An experiment is carried out where [A] = 1.0 x 10-2 M, [B] = 8.0 M, and [C] = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 × 10-³ M. a. Calculate the value of k for this reaction. -2-1 L² mol s b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 14.0 seconds. Concentration = M d. Calculate the concentration of C after 14 seconds. Concentration = M

Consider the hypothetical reaction A+B+ 2C 2D+3E where the rate law is Rate =- Δ[Α] At k= = k[A][B]² = An experiment is carried out where [A] = 1.0 x 10-2 M, [B] = 8.0 M, and [C] = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 × 10-³ M. a. Calculate the value of k for this reaction. -2-1 L² mol s b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 14.0 seconds. Concentration = M d. Calculate the concentration of C after 14 seconds. Concentration = 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 = A[A] At k= An experiment is carried out where [A] = 1.0 × 10-² a. Calculate the value of k for this reaction. -2 L² mol s = k[A][B]² Concentration = b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 14.0 seconds. M d. Calculate the concentration of C after 14 seconds. Concentration = S -1 M M, [B] = 8.0 M, and [C]o = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 × 10-³ M.
Transcribed Image Text:Consider the hypothetical reaction A+B+ 2C 2D+3E where the rate law is Rate = A[A] At k= An experiment is carried out where [A] = 1.0 × 10-² a. Calculate the value of k for this reaction. -2 L² mol s = k[A][B]² Concentration = b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 14.0 seconds. M d. Calculate the concentration of C after 14 seconds. Concentration = S -1 M M, [B] = 8.0 M, and [C]o = 2.0 M. The reaction is started, and after 7.0 seconds, the concentration of A is 3.8 × 10-³ M.
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