The rate for the oxidation of iron(II) by cerium(IV) Ce** (aq) + Fe²* (aq) → Ce* (aq) + Fe* (aq) is measured at several different initial concentrations of the two reactants: [Ce**] (mol L-') [Fe?+] (mol L-') Rate (mol L-s-') 1.1 x 10-5 1.8 x 10-5 2.0 x 10-7 1.1 x 10-5 2.8 x 10-5 3.1 x 10-7 3.4 x 10-5 2.8 x 10-5 9.5 x 10-7 (a) Write the rate expression for this reaction. (b) Calculate the rate constant k and give its units. (c) Predict the initial reaction rate for a solution in which [Ce**] is 2.6 x 10-5 M and [Fe²*] is 1.3 × 10-5 M.

The rate for the oxidation of iron(II) by cerium(IV) Ce** (aq) + Fe²* (aq) → Ce* (aq) + Fe* (aq) is measured at several different initial concentrations of the two reactants: [Ce] (mol L-') [Fe?+] (mol L-') Rate (mol L-s-') 1.1 x 10-5 1.8 x 10-5 2.0 x 10-7 1.1 x 10-5 2.8 x 10-5 3.1 x 10-7 3.4 x 10-5 2.8 x 10-5 9.5 x 10-7 (a) Write the rate expression for this reaction. (b) Calculate the rate constant k and give its units. (c) Predict the initial reaction rate for a solution in which [Ce] is 2.6 x 10-5 M and [Fe²*] is 1.3 × 10-5 M.

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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