7 of 18 I Review | Constants | Periodic Tab Analyzing a new reaction Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. Consider the following elementary steps that make up the mechanism of a certain reaction: 1.3XE +F 2. E + MF +N Very often, a reaction does not tell us the whole story. For instance, the reaction Part A NO2(9) + CO(g)-→NO(9) + CO2(9) does not involve a collision between an NO2 molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: What is the overall reaction? Express your answer as a chemical equation. > View Available Hint(s) 1. NO2(9) + NO2(9)→NO3(9) + NO(g) 2. NO3(9) + CO(9)→CO2(9) + NO2(9) ΑΣφ ? Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. Overall, the resulting reaction is DA chemical reaction does not occur for this question. NO2(9) + CO(g)→NO(g) + CO2(9) Submit Notice that in the elementary steps NO3 appears

7 of 18 I Review | Constants | Periodic Tab Analyzing a new reaction Learning Goal: To understand how elementary steps make up a mechanism and how the rate law for an elementary step can be determined. Consider the following elementary steps that make up the mechanism of a certain reaction: 1.3XE +F 2. E + MF +N Very often, a reaction does not tell us the whole story. For instance, the reaction Part A NO2(9) + CO(g)-→NO(9) + CO2(9) does not involve a collision between an NO2 molecule and a CO molecule. Based on experimental data at moderate temperatures, this reaction is thought to occur in the following two steps: What is the overall reaction? Express your answer as a chemical equation. > View Available Hint(s) 1. NO2(9) + NO2(9)→NO3(9) + NO(g) 2. NO3(9) + CO(9)→CO2(9) + NO2(9) ΑΣφ ? Each individual step is called an elementary step. Together, these elementary steps are called the reaction mechanism. Overall, the resulting reaction is DA chemical reaction does not occur for this question. NO2(9) + CO(g)→NO(g) + CO2(9) Submit Notice that in the elementary steps NO3 appears

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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Using the data in the table, calculate the rate constant of this reaction. k= = A + B → C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.340 0.400 0.340 0.920 0.408 0.400 Rate (M/s) 0.0114 0.0603 0.0137
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A chemistry graduate student is studying the rate of this reaction: 2C1,O, (g) 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. [C1,05] 40. 0.600M 0.172M 0.101 M 30. 0.0710M 0.0548M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X Ś
The data for the reaction given NOCI (g) The following experimental data was measured for the reaction. Use the Method of Initial Rates to determine the rate law equation for this reaction 1 2 3 NO (g) + 1/2 Cl2₂ (g) [NO] [Cl₂] Initial Rate Experiment (mol.L-¹) (mol.L-¹) (mol.L-¹ s¯¹) 1.4x10-6 2.8x10-6 5.6x10-6 0.250 0.250 0.500 0.250 0.500 0.250 → 1. Determine the order of the reaction with respect to NO oxide 2. Determine the order of the reaction with respect to Cl₂ 3. What is the overall order of this reaction? 5. Calculate the value of the rate constant, k → 4. Select the correct rate law (rate equation) for this reaction: Rate =
Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A](M) 0 0.5 1.5 0.42 3 0.335 4.5 0.25 6 0.17 7.5 0.085 9 0.003
The following kinetic data were obtained for the reaction A (g) + 2 B (g) → products Trial [A] (M) [B] (M) Initial Rate (M s-1) 1 0.60 0.30 0.0126 2 0.20 0.30 0.0014 3 0.60 0.10 0.0042 Determine the order with respect to A. Enter the answer as a single digit, not the word.
Consider the gas phase reaction 2 NO + H₂ → N₂O + H₂O The experimental rate law is found to be R = [NO]²[H₂] Which of the mechanisms shown below is consistent with the information about this reaction given in this question? Step 1: NO + H₂ → N + H₂O (slow) Step2: N + NO → N₂O (fast) Step 1: NO + NO 2 NO₂ + N (slow) (fast) Step2: NO₂ + H₂ Step 3: N + NO → NO + H₂O N₂O (fast) Step 1: NO + NO>>> N₂O₂ Step2: N₂O₂ + H2 →→ N₂O + H₂O 2H (fast) Step 1: H₂ Step2: H+2 NO → Step 3: H+ OH → N₂O + OH (slow) H₂O (fast) (fast) (slow)