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O₂(g) + NO(g) →→→ O₂(g) + NO₂ ate law for this reaction is rate of reaction = k[03][NO] that k = 4.42 x 106 M-¹.s-¹ at a tially constant at the values [03] ate sources.

O₂(g) + NO(g) →→→ O₂(g) + NO₂ ate law for this reaction is rate of reaction = k[03][NO] that k = 4.42 x 106 M-¹.s-¹ at a tially constant at the values [03] ate sources.

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 reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by 03(g) + NO(g) O₂(g) + NO₂ (g) The rate law for this reaction is rate of reaction = k[03][NO] Given that k = 4.42 × 106 M-¹-s¯¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03]o = 3.22 × 10-6 M and [NO]。 = 5.48 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h¹.L-1
Transcribed Image Text:A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by 03(g) + NO(g) O₂(g) + NO₂ (g) The rate law for this reaction is rate of reaction = k[03][NO] Given that k = 4.42 × 106 M-¹-s¯¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03]o = 3.22 × 10-6 M and [NO]。 = 5.48 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h¹.L-1
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