The rate constant for the formation of hydrogen iodide from the elements H₂(g) + I₂(g) → 2HI(g) L/(mol.s) at 600 K and 3.5 × 10-³ L/(mol·s) at 650 K. a. Find the activation energy Ea. J/mol b. Then calculate the rate constant at 685 K. L/(mol.s) is 2.7 x 10-4
The rate constant for the formation of hydrogen iodide from the elements H₂(g) + I₂(g) → 2HI(g) L/(mol.s) at 600 K and 3.5 × 10-³ L/(mol·s) at 650 K. a. Find the activation energy Ea. J/mol b. Then calculate the rate constant at 685 K. L/(mol.s) is 2.7 x 10-4
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 23P
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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 10-4 L/(mol·s) at 600 K and 3.5 × 10-³ L/(mol·s) at 650 K.
a. Find the activation energy Ea.
J/mol
b. Then calculate the rate constant at 685 K.
L/(mol.s)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ea83443-9d3f-459e-ba66-94134a3e3adc%2F4bd6ea73-8474-4465-a5af-8eced4b9b9ea%2F7c6fs7_processed.png&w=3840&q=75)
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 10-4 L/(mol·s) at 600 K and 3.5 × 10-³ L/(mol·s) at 650 K.
a. Find the activation energy Ea.
J/mol
b. Then calculate the rate constant at 685 K.
L/(mol.s)
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