Which of the following is true? A) If we know that a reaction is an elementary reaction, then we know its rate law. B) The rate-determining step of a reaction is the rate of the fastest elementary step of its mechanism. C) Since intermediate compounds can be formed, the chemical equations for the elementary reactions in a multistep mechanism do not always have to add to give the chemical equation of the overall process. D) All of the above statements are true.

Which of the following is true? A) If we know that a reaction is an elementary reaction, then we know its rate law. B) The rate-determining step of a reaction is the rate of the fastest elementary step of its mechanism. C) Since intermediate compounds can be formed, the chemical equations for the elementary reactions in a multistep mechanism do not always have to add to give the chemical equation of the overall process. D) All of the above statements are true.

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...

See similar textbooks

Similar questions

Compounds A and B react to give a single product, C. Write the rate law for each of the following cases and determine the units of the rate constant by using the units M for concentration and s for time: (1) The reaction is first order in A and second order in B. Rate= Units: (2) The reaction is first order in A and second order overall. Rate= Units: (3) The reaction is independent of the concentration of A and second order overall. Rate= Units: (4) The reaction is second order in both A and B. Rate= Units:
Deducing a rate law from the change in concentration over time A chermistry graduate student is studying the rate of this reaction: Н,Со, (аg) - н,о (аq) +со, (aqg) She fills a reaction vessel with H,Co, and measures its concentration as the reaction proceeds: olo time [H,CO,] (seconds) 0.0200M 10. 0.00577M 20. 0.00337M 30. 0.00238 M 40. 0.00184M Use this data to answer the following questions. Write the rate law for this reaction. rate = k || Ox10 Calculate the value of the rate constant k. k = 0 Round your answer to 2 significant digits. Also be ? sure your answer has the correct unit symbol. ||
Use the kinetic theory to justify the observation that the rate of a reaction in the gas phase depends on the energy of the two molecules that collide.
Obtain the rate law based on the kinetic study of the reaction.
For a given chemical reaction that only involves compound A, changing the concentration of [ A ] = 0.333 M to [ A ] = 0.499 changes the rate from 4.2 M/s to 6.3 M/s. What is the best rate law for this reaction and the value of the rate constant?
3. The rate data were obtained in a series of experiments for the reaction at a particular temperature. 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) Experiment Initial [NO] (M) 0.22 0.22 Initial (H2] (M) 0.12 0.24 Rate of Appearance of N2 (Ms1) 0.033 1 2 0.066 3 0.44 0.12 0.132 (a) From these data, determine: (i) (ii) (iii) the rate law for the reaction the order of reaction the rate constant. (b) How is the rate of this reaction affected by each of the following changes? (i) (i) the concentration of NO is quadrupled the concentration of H2 is doubled and NO is tripled. (c) What is the rate of formation of N2 when [NO] is 0.14 mol L-1 and [H2] is 0.12 mol L1?
Here is a graph of the molarity of thionyl chloride (SOC1,) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. 0.003 0.00254 0.002 M 0.001 %23 500 1000 1500 2000 2500 3000 seconds created x10 Is SOCI, being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If SOCI, is being created or destroyed, what is the rate at which it is being created or destroyed 800 seconds after the reaction starts? 511A Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility MacBook Air O00 000 DII
1. What is meant by the rate determining step in a reaction mechanism?
Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g) → 2C1, (g) + 50, (g) He fills a reaction vessel with Ci,0, and measures its concentration as the reaction proceeds: time [C1,0,] (seconds) 0.0500M 10. 0.0170M 20. 0.0103 M 30. 0.00735 M 40. 0.00573 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Calçulate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be ? sure your answer has the correct unit symbol.
The decomposition of NO2 produces NO gas and oxygen gas. The decomposition is determined to occur at half-lives of 12, 24, and 48 seconds. If the pressure of NO₂ is initially 746 torr in a 5.00L container at 383°C a) Write the rate law for the reaction b) What is the molar concentration of NO2 after 24 seconds c) What is the molar concentration of NO2 after 96 seconds
7 . Please make sure the answer that you give me is correct thank you
Consider the following reaction: Cl2O (g) + CO (g) → Cl2 (g) + CO2 (g) Initial rate of the reaction was measured at multiple different concentrations of CO, which created the following data: [CO] (M) Initial Rate (M/s) 0.10 0.0020 0.20 0.0040 0.40 0.0080 From this data, we can see that the reaction order with respect to CO is __________. Consider the following reaction: Cl2O (g) + CO (g) → Cl2 (g) + CO2 (g) Initial rate of the reaction was measured at multiple different concentrations of CO, which created the following data: From this data, we can see that the reaction order with respect to CO is __________. a. 1st Order b. 3rd Order c. 2nd Order d. 0th Order