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Provide the answers to the following questions. Show all of your work with correct units throughout your calculations and final answers. Box or circle your final answer. 1. Given the following reaction: N½O5 (g) → NO2 (g) + O2 (g) 1. Write the rate if reaction in terms of the change in concentration of N,Os. 2. Write the rate of formation of NO2 and 02 in terms of N205. Second Ouestion

Provide the answers to the following questions. Show all of your work with correct units throughout your calculations and final answers. Box or circle your final answer. 1. Given the following reaction: N½O5 (g) → NO2 (g) + O2 (g) 1. Write the rate if reaction in terms of the change in concentration of N,Os. 2. Write the rate of formation of NO2 and 02 in terms of N205. Second Ouestion

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 12QRT: Cyclobutane can decompose to form ethylene: The cyclobutane concentration can be measured as a...
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First Homework First Question Provide the answers to the following questions. Show all of your work with correct units throughout your calculations and final answers. Box or circle your final answer. 1. Given the following reaction: N205 (g) → NO2 (g) + 02 (g) 1. Write the rate if reaction in terms of the change in concentration of N205. 2. Write the rate of formation of NO2 and O2 in terms of N205. Second Question A+B →C +D [B]o, M Initial Rate, M/min 0.0010 Experiment [A]o, M 1 1.0 1.0 2 3.0 1.0 0.0030 3 1.0 2.0 0.0020 Write the order for each reactant and the experiment rate law? Fourth Question For a first order process, the initial concentration of A is 0.816 M and the concentration of A after 16 minutes is 0.632 M. A. Is A a reactant or product? Justify. B. What is the rate constant for this reaction? C. What is the half life? D. How many minutes must pass before [A] = 0.235M E. What is the concentration of A after 2.5 hours? Fifth Question Using the following data for the reaction A->B, Time, sec [A], M 1.00 50 0.67 100 0.50 150 0.40 200 0.33 250 0.29 1. Construct a zero, first, and second order graph. This can be hand-drawn or computed on Excel. 2. Is this reaction that is occurring zero, first, or second order? Justify. 3. What is the rate constant of the reaction? 4. Determine the experimental rate law
Transcribed Image Text:First Homework First Question Provide the answers to the following questions. Show all of your work with correct units throughout your calculations and final answers. Box or circle your final answer. 1. Given the following reaction: N205 (g) → NO2 (g) + 02 (g) 1. Write the rate if reaction in terms of the change in concentration of N205. 2. Write the rate of formation of NO2 and O2 in terms of N205. Second Question A+B →C +D [B]o, M Initial Rate, M/min 0.0010 Experiment [A]o, M 1 1.0 1.0 2 3.0 1.0 0.0030 3 1.0 2.0 0.0020 Write the order for each reactant and the experiment rate law? Fourth Question For a first order process, the initial concentration of A is 0.816 M and the concentration of A after 16 minutes is 0.632 M. A. Is A a reactant or product? Justify. B. What is the rate constant for this reaction? C. What is the half life? D. How many minutes must pass before [A] = 0.235M E. What is the concentration of A after 2.5 hours? Fifth Question Using the following data for the reaction A->B, Time, sec [A], M 1.00 50 0.67 100 0.50 150 0.40 200 0.33 250 0.29 1. Construct a zero, first, and second order graph. This can be hand-drawn or computed on Excel. 2. Is this reaction that is occurring zero, first, or second order? Justify. 3. What is the rate constant of the reaction? 4. Determine the experimental rate law
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