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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 = 2.71 × 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]0 = 5.56 × 10-6 M and [NO]o = 6.37 x 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

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 = 2.71 × 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]0 = 5.56 × 10-6 M and [NO]o = 6.37 x 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

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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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 = 2.71 × 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]0 = 5.56 × 10-6 M and [NO]o = 6.37 x 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 = 2.71 × 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]0 = 5.56 × 10-6 M and [NO]o = 6.37 x 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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