The following reaction in aqueous solution was found to be first order in [OH-], first order in [C₂H5Br], and inverse first order in Br C₂H5Br + OH-C₂H5OH + Br Which one of the following mechanisms is consistent with the observed reaction order? C₂H5OHC₂H5OH (slow) C₂H5Br C₂H5 + Br (fast) C₂H5Br C₂H5+ Br C₂H5OHC₂H5OH C₂H5Br C₂H5 + Br OH+Br-HOBr HOBr +C₂H5 C₂H5OH+Br (fast) (slow) (fast) (slow) (fast) C₂H5Br +H₂O-C₂H5OH+H+Br (slow) H* + OH-H₂O (fast)

The following reaction in aqueous solution was found to be first order in [OH-], first order in [C₂H5Br], and inverse first order in Br C₂H5Br + OH-C₂H5OH + Br Which one of the following mechanisms is consistent with the observed reaction order? C₂H5OHC₂H5OH (slow) C₂H5Br C₂H5 + Br (fast) C₂H5Br C₂H5+ Br C₂H5OHC₂H5OH C₂H5Br C₂H5 + Br OH+Br-HOBr HOBr +C₂H5 C₂H5OH+Br (fast) (slow) (fast) (slow) (fast) C₂H5Br +H₂O-C₂H5OH+H+Br (slow) H* + OH-H₂O (fast)

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

The reaction: A + 3B-> D + F was studied and the following mechanism was determined A + B -> C (fast) C + B-> D + E (slow) E + B -> F (very fast) The step with largest activation energy is None of the steps has an activation energy. the first step the third step All steps have the same activation energy. the second step
Consider the first-order reaction described by the equation HH H.C- CCH, H-C- -с —н H H Cyclopropane Propene At a certain temperature, the rate constant for this reaction is 5.84 × 104 s-!. Calculate the half-life of cyclopropane at this temperature. 12 = S Given an initial cyclopropane concentration of 0.00700 M, calculate the concentration of cyclopropane that remains after 1.70 hours. concentration:
The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,Og) —CH,(g) +CO(g) Verify that this is a first-order reaction by plotting In[C,H,O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 52.0 75.0 97.0 135.0 k == min!
What percentage of the initial amount of S02Cl2 2ilk remain after 2.25 hours?
For a hypothetical reaction qQ Ra graph of the experimental data of 1/[Q] versus time is linear. What is the reaction order with respect to the reactant (Q)? O First-order O Zero-order O Third-order O Second-order O Fourth order O None of the above
What is the half-life of a 1st order reaction whose rate law constant is 3.7x10-2s-1? 5.3x10-2seconds 19 seconds 2.6x10-2seconds 39 seconds
A reaction is second order with respect to reactant "A" and has a rate constant of 2.97 x 10-2 M-1s-1. If the initial concentration of A is 0.100 M, what will the concentration drop to after 30.0 minutes? 6.06 x 10E(-25) M 9.18 x 10E(-2) M 1.58 x 10E(-2) M 1.01 x 10E(-26) M
The following reaction was studied at a given temperature: CH3CI(g) + H20(g) → CH3OH(g) + HCI(g) From the rate data below, determine the reaction orders. Exp [CH3CI]o [H2O]o Initial Rate (M s1) 1 0.100 0.100 0.182 2 0.200 0.200 1.45 3 0.200 0.400 5.81 CH3CI: first order H2O: first order CH3CI: second order H,O: second order CH3CI: second order H,O: first order O CH3CI: first order H2O: second order
During kinetic studies, the following reaction was determined to be first order in respect to CH3OH and second order in respect to HCl. What is the overall order for the reaction? CH3OH(aq) + HCl(aq) ----> CH3Cl(aq) + H2O(i)
The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,Og) —CH,(g)+CO(g) Verify that this is a first-order reaction by plotting In[C,H,O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 50.0 72.0 93.0 130.0 min
A particular second order reaction has a rate constant of 0.0345 M-1 min-1 and an initial concentration of 0.300 M. What is the half-life of this reaction? 4.35 min 12.0 min 20.1 min 96.6 min
A chemistry graduate student is studying the rate of this reaction: NH₂OH(aq) → NH3 (aq) +H₂O (aq) She fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds: time (milliseconds) 0 [NHẠOH] 0.0400M 10. 0.0126M 20. 0.00748M 30. 0.00532 M 40. 0.00413 M 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 X Ś