Consider the following proposed reaction mechanism: Step 1: F2 + 2 NO2 → NO2F + F + NO2 Step 2: F + NO2 → NO2F The first step is the slow (rate-determining) step. Answer the following questions: Question 29: The reactants in the overall equation are (including their correct coefficients): NO2 NO₂F 2 F2 2 NO2 2 F F2 F 2 NO2F Check

Consider the following proposed reaction mechanism: Step 1: F2 + 2 NO2 → NO2F + F + NO2 Step 2: F + NO2 → NO2F The first step is the slow (rate-determining) step. Answer the following questions: Question 29: The reactants in the overall equation are (including their correct coefficients): NO2 NO₂F 2 F2 2 NO2 2 F F2 F 2 NO2F Check

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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#8
Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.912M 2.49 M 18.0M/s 0.374M 2.49 M 0.912M 11.2 M Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k 3.03 M/s 364. M/s k = ☐ x10 ロ・ロ X
Try Again Your answer is incorrect. • Row 2: Your answer is incorrect. Please check your units. Some measurements of the initial rate of a certain reaction are given in the table below. N₂ H₂] initial rate of reaction 0.945 M 1.74M 1.00 × 106 M/s 0.945M 0.395M 5.15 × 10+ M/s 0.458M 1.74M 4.85 × 105 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k [N,][H, 5 k 3.5 X 10 - 2 - 1 M S x10 Ś
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
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How would each of the following change the rate of the reaction shown here? Drag the appropriate items to their respective bins. decreasing the temperature adding some NO(g) Reaction rate increases 2NO(g) + 2H₂(g) → N2(g) + 2H₂O(g) Submit Request Answer Reaction rate decreases removing some H₂(g) P Pearson adding a catalyst Reset Help Reaction rate remains the same.
Question 12 Which of the following best describes the rate law? O A theoretical equation that describes how the rate of reaction depends on temperature, orientation and number of collisions. O A theoretical equation that describes how the rate of reaction depends on the concentration of reactants. O An experimentally determined equation that describes how the rate of reaction depends on temperature, orientation and number of collisions. O An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants.
Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased
Question 36 of 42 For the theoretical reaction 2A →C the reaction mechanism was determined to be 1. A+A → B 2. B-C This reaction also follows the reaction profile below. Potential Energy Reaction Coordinate The rate determining step of this reaction is step Step 1 Step 2 Unable to determine
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.
6. A student performs the reaction below in three experiments studying initial concentrations and initial rates. The data is summarized in the table below. SHOW ALL YOUR WORK. 2 NO(g) + Br₂(g) →2 NOBr(g) [NO] 0.80 1.60 0.80 [Br.] 0.60 0.60 1.20 Rate (mol/L.s) 0.14 0.28 0.56 a. What is the order of this reaction with respect to NO? b. What is the order of this reaction with respect to Br₂? c. What is the overall order of this reaction? d. What is the rate law constant, k, for this reaction? (Be sure to include the value and the units.)
Question 9 Which of the following statements is false? The average rate of a reaction decreases during a reaction. It is not possible to determine the rate of a reaction from its balanced equation. The rate of zero order reactions is not dependent on concentration. The half-life of a first order reaction is dependent on the initial concentration of reactant. None of the statements are false.