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The rate constant for the formation of hydrogen iodide from the elements H2(g) + I2(g) → 2HI(g) is 2.7 x 10 L/(mol-s) at 600 K and 3.5 × 10 3 L/(mol-s) at 650K. a. Find the activation energy E. 166000 V J/mol b. Then calculate the rate constant at 678 K. *L/(mol•s)

The rate constant for the formation of hydrogen iodide from the elements H2(g) + I2(g) → 2HI(g) is 2.7 x 10 L/(mol-s) at 600 K and 3.5 × 10 3 L/(mol-s) at 650K. a. Find the activation energy E. 166000 V J/mol b. Then calculate the rate constant at 678 K. *L/(mol•s)

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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The rate constant for the formation of hydrogen iodide from the elements H2(g) + I2(g) → 2HI(g) is 2.7 x 104 L/(mol·s) at 600 K and 3.5 × 103 L/(mol-s) at 650 K. a. Find the activation energy E. 166000 V J/mol b. Then calculate the rate constant at 678 K. * L/(mol•s)
Transcribed Image Text:The rate constant for the formation of hydrogen iodide from the elements H2(g) + I2(g) → 2HI(g) is 2.7 x 104 L/(mol·s) at 600 K and 3.5 × 103 L/(mol-s) at 650 K. a. Find the activation energy E. 166000 V J/mol b. Then calculate the rate constant at 678 K. * L/(mol•s)
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