QUESTION 13Given the reaction2N 20 5(g) → 4NO 2(g) + O 2(g),the rate of reaction based on N 20 5(g) is correctly written asateate = - 2%3Date =rate = -AN205]Click Save and Submit to save and submit. Click Save All Answers to save all answers.MacBook Air

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Answered: QUESTION 13 Given the reaction 2N 20…

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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QUESTION 5 Fo O319) → NO2(9) + For the reaction NO) + O2(9) the value of A= 8.7 x 1012 s-1 and Ea = 63 kJ/mol. %3D What is the value of the rate constant k for the reaction at 75°C? Enter your answer in units of s to 2 significant figures. Enter your answer in the format: a.b x10^m, where a.b and m are the appropriate numbers based on your calculation.
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14 9 12 15 Question 12 Listen If dinitrogen pentoxide decomposes as follows: 2 N₂05(g) - 4 NO2(g) + O₂(g) If the reaction rate is expressed as: rate = k [N₂O5]¹, then the overall reaction order is: (Enter your answer as a number. (i.e. as "5" not "five")) Your Answer: Answer
Consider the balanced reaction below. 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g) a) Write the relative rate expression for the reaction (including each of the reactants and products). b) If the rate of N2H4 consumption is 0.50 M/s, what is the rate of N2 production? Show your work or explain your reasoning.
QUESTION 2 The following mechanism has been proposed for the gas-phase exothermic reaction of chloroform (CHCl3) and chlorine: Step 1: Step 2: Step 3: Q 2(a) Cl₂2Cl Cl + CHCl3 → HCl+ CCl3 Cl + CCl3 → CCl4 i. What is the overall reaction? (fast) (slow) (fast) ii. What are the intermediates in the mechanism? iii. What is the molecularity of the elementary reactions? iv. Write down the rate law for each elementary reaction. v. What is the rate-determining step? Q 2(b) Using the rate-determining step and pre-equilibria determine the rate law predicted by this mechanism. Q2(c) Roughly sketch and label a reaction profile graph (potential energy vs reaction coordinate) for this reaction. ii. Include in the graph: reactants, products, intermediary/intermediaries, activation energy for each elementary step. iii. Compare the activation energy for all the elementary step, indicating which one is the highest.
4. Given the following balanced equation, determine the rate of reaction with respect to [NOCI]. If the rate of Cl₂ loss is 4.84 × 10-2 M/s, what is the rate of formation of NOCI? 2 NO(g) + Cl2(g) → 2 NOCI(g) A. 4.84 x 10-2 M/s B. 2.42 x 102 M/s C. 1.45 × 10-1 M/s D. 9.68 × 10-2 M/s E. 1.61 × 102 M/s
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…
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Question 13 of 32 Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is Rate [A], (M) [B], (M) (M/s) A) Rate = k[A][B] 0.100 2.50 0.460 B) Rate = k[B] C) Rate = k[A]°[B] 0.200 2.50 0.920 D) Rate = k[A] 0.300 1.25 1.38 "pe here to search
60 QUESTION 13 The following graphs can be used for the questions that follow: 00 B0 00 Seris 1 02 time(min) D2 -D4 y = -0.0358x + 0.1058 Liner (Serive t) -18 time(min) The decomposition reaction of NO 2 is important in atmospheric chemistry. The reaction 2NO 2(g) → 2NO(g) + O 2(g) is second order with respect to NO 2. How can the rate constant be determined? A plot of 1/[NO2] versus time will be linear with a slope of -k. A plot of 1/[NO2] versus time will be linear with a slope of k. A plot of [NO2] versus time will be linear with a slope of -k. A plot of In[NO2] versus time will be linear with a slope of -k. Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air DD F8 F3 F4 F5 F1 %23 24 2 4. 7.

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QUESTION 13 Given the reaction 2N 20 5(g) → 4NO 2(g) + O 2(g), the rate of reaction based on N 20 5(g) is correctly written as ate ate = - 2 %3D ate = rate = - AN205] Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air