Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.420 0.733 0.0145 Trial 2 0.840 0.733 0.0579 Trial 3 0.420 1.47 0.0290 Trial 4 0.827 0.710 0.0544 Rate = k[A]°[B]! X L/mol•min Recheck Next (5 of 5) 8th attempt
Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.420 0.733 0.0145 Trial 2 0.840 0.733 0.0579 Trial 3 0.420 1.47 0.0290 Trial 4 0.827 0.710 0.0544 Rate = k[A]°[B]! X L/mol•min Recheck Next (5 of 5) 8th attempt
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 30E: The reaction 2I-(aq)+S2O82-(aq)I2(aq)+2SO42-(aq) was studied at 25C. The following results were...
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Now that the order for both reactants is known, the rate constant, k, can be determined.
Each of the four trials can be used to calculate k and then the four results can be averaged.
We will use Trial 4 to determine the rate constant in this example.
What is the value of the rate constant?
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