Experimental Data Table: Initial [IO3¯ ag] (mol/L) Initial [H* Initial [I (ag)] (mol/L) Trial Run Time to react (ag)] (mol/L) (seconds) 1 0.005 0.00002 0.05 18.4 2 0.005 0.00004 0.05 5.4 3 0.01 0.00004 0.05 3.1 4 0.01 0.00002 0.05 9.6 5 0.01 0.00002 0.1 3.3 6 0.02 0.00002 0.1 2.0 7 0.02 0.00001 0.1 5.2 8 0.02 0.00001 0.15 3.0 Analyze and Evaluate: (a) Identify the orders of reaction for IO3", H*, and I-. (b) What is the total order of reaction? (c) Write the rate law equation for this iodine clock reaction. You do not need to calculate the value of the rate constant.

Experimental Data Table: Initial [IO3¯ ag] (mol/L) Initial [H* Initial [I (ag)] (mol/L) Trial Run Time to react (ag)] (mol/L) (seconds) 1 0.005 0.00002 0.05 18.4 2 0.005 0.00004 0.05 5.4 3 0.01 0.00004 0.05 3.1 4 0.01 0.00002 0.05 9.6 5 0.01 0.00002 0.1 3.3 6 0.02 0.00002 0.1 2.0 7 0.02 0.00001 0.1 5.2 8 0.02 0.00001 0.15 3.0 Analyze and Evaluate: (a) Identify the orders of reaction for IO3", H*, and I-. (b) What is the total order of reaction? (c) Write the rate law equation for this iodine clock reaction. You do not need to calculate the value of the rate constant.

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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