Consider the hypothetical reaction A +B+ 2C –→ 2D + 3E where the rate law is A[A] = k[A][B]? At Rate = %3D An experiment is carried out where = 1.0 x 10¬2 M. [A], = (B], 6.0 М, and [C], = 2.0 M. The reaction is started, and after 5.0 seconds, the concentrati A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mols-1 b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = M d. Calculate the concentration of C after 19 seconds. Concentration =

Consider the hypothetical reaction A +B+ 2C –→ 2D + 3E where the rate law is A[A] = k[A][B]? At Rate = %3D An experiment is carried out where = 1.0 x 10¬2 M. [A], = (B], 6.0 М, and [C], = 2.0 M. The reaction is started, and after 5.0 seconds, the concentrati A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mols-1 b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = M d. Calculate the concentration of C after 19 seconds. Concentration =

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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A+ B+ 2C - 2D+ 3E where the rate law is A[A] k[A][B]* Rate = - %3D At An experiment is carried out where [A], = 1.0 x 10-2 M, [B, = 6.0 M, and [C, = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k%3= L mols 1 b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 17.0 seconds. Concentration= M d. Calculate the concentration of C after 17 seconds. Concentration=