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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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A student obtained the following data for the decomposition of hydrogen iodide on a gold surface at 150 °C. HI(g) 12 H₂(g) + ½ I₂(g) [HI], M seconds 0.140 ♥ 0 7.00×10-² 521 3.50×10-2 781 1.75×10-2 (1) What is the half-life for the reaction starting at t=0 s? What is the half-life for the reaction starting at t=521 s? Does the half-life increase, decrease or remain nstant as the reaction proceeds? (2) Is the reaction zero, first, or second order? 911 S (3) Based on these data, what is the rate constant for the reaction? S Ms-1
Transcribed Image Text:A student obtained the following data for the decomposition of hydrogen iodide on a gold surface at 150 °C. HI(g) 12 H₂(g) + ½ I₂(g) [HI], M seconds 0.140 ♥ 0 7.00×10-² 521 3.50×10-2 781 1.75×10-2 (1) What is the half-life for the reaction starting at t=0 s? What is the half-life for the reaction starting at t=521 s? Does the half-life increase, decrease or remain nstant as the reaction proceeds? (2) Is the reaction zero, first, or second order? 911 S (3) Based on these data, what is the rate constant for the reaction? S Ms-1
The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g)+½O₂(g) is second order in NO₂ with a rate constant of 0.540 1 M.S If the initial concentration of NO2 is 0.112 M, the concentration of NO₂ will be 2.31 x 10-2 M after seconds have passed.
Transcribed Image Text:The gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) → NO(g)+½O₂(g) is second order in NO₂ with a rate constant of 0.540 1 M.S If the initial concentration of NO2 is 0.112 M, the concentration of NO₂ will be 2.31 x 10-2 M after seconds have passed.
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