mical Kinetics Workbook 2022.docx(b) (A.C. 2.2)The initial rate of the reaction between substances A andB was measured in a further series of experiments and thefollowing rate equation was deduced.rate = K[A][B]2(i) Complete the table of data below for the reactionbetween A and B.Expt1234= Open with Google DocsLOInitial [A]/mol dm-30.0200.0400.0600.040Initial [B]/mol dm-30.0200.0400.0400.030Initial rate/mol dm-3 s-1+1.2x10-42.4×10-47.2x10-4(ii) Using the data for Experiment 1, calculate a value forthe rate constant, k and state its units.Page 5 / 6Q

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(b) (A.C. 2.2) The initial rate of the reaction between substances A and B was measured in a further series of experiments and the following rate equation was deduced. rate = K[A][B]2 (i) Complete the table of data below for the reaction between A and B. Expt 1 2 3 4 5 Initial [A] /mol dm-3 0.020 0.040 0.060 0.040 Initial [B] /mol dm-3 0.020 0.040 0.040 0.030 Initial rate /mol dm-3 s-1 1.2x10-4 2.4×10-4 7.2x10-4 Using the data for Experiment 1, calculate a value for the rate constant, k and state its units. Page 5/6 Q +

(b) (A.C. 2.2) The initial rate of the reaction between substances A and B was measured in a further series of experiments and the following rate equation was deduced. rate = K[A][B]2 (i) Complete the table of data below for the reaction between A and B. Expt 1 2 3 4 5 Initial [A] /mol dm-3 0.020 0.040 0.060 0.040 Initial [B] /mol dm-3 0.020 0.040 0.040 0.030 Initial rate /mol dm-3 s-1 1.2x10-4 2.4×10-4 7.2x10-4 Using the data for Experiment 1, calculate a value for the rate constant, k and state its units. Page 5/6 Q +

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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The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.
(a) For the generic reaction A ---> B. If this is a first-order reaction, what quantity when graphed versus time will yield a straight line? (b) how can you calculate the rate constant for the first-order reaction from the graph you made in part (a)? Group of answer choices A.) (a) a graph on log[A] versus time yields a straight line for a first-order reaction. (b) the slope of the straight line. B.) (a) a graph on 1/[A] versus time yields a straight line for a first-order reaction. (b) the slope of the straight line. C.) (a) a graph on [A] versus time yields a straight line for a first-order reaction. (b) the slope of the straight line. D.) (a) a graph on ln[A] versus time yields a straight line for a first-order reaction. (b) the negative slope of the straight line.
4.) The overall reaction 2NO2(g) + F2(g) →2NO2F(g) has an experimental rate law Rate = k[NO2][F2]. The accepted two step mechanism is: %3D (1) NO2(g) + F2(g) → NO2F(g) + F(g) (2) NO2(g) + F(g) → NO,F(g) [slow; rate determining] [fast] a. Write the rate laws for each of the elementary steps. b. What is the molecularity for each step? C. Show how the elementary steps sum to the overall balanced equation: d. Which species (if any) are intermediates? Which step is rate-limiting? e. f. Is the mechanism reasonable and consistent with the observed rate law? Explain
1. Consider the reaction for the production of urea used in synthesizing fertilizers: Answer the following. + 2NH30) CO2 (9) CO(NH,)2() + H200) During the analysis, a student found that the rate of ammonia consumption is 5.45 x 103 What was the rate (a) CO, was reacting? (b) CO(NH,), was being formed? (c) H,0 was being produced?
[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.
Write the reaction rate expressions for the following reactions in terms of the disappearance of the reactants and the appearance of products: (a) H2(g) + I2(g) ⟶ 2HI(g) (b) 5Br−(aq) + BrO−3 (aq) + 6H+(aq) ⟶ 3Br2(aq) + 3H2O(l)
For the reaction: 2A + B -->C, the rate of formation of C was measured for a number of different initial concentrations of A and B, with the following results a)Determine the rate law. b) Calculate the rate constant. c) Suggest a two-step mechanism that is consistent with the experimental data.
The reaction 2 NO(g) + O₂(g) -> 2 NO₂(g) proceeds through the following mechanism: (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Ratek [NO] (O₂) Rate-k [NO] [0₂] Ratek [NO] [O₂)² Ratek [NO]1/2 [0₂] Ratek [NO] [0₂]1/2 O Rate-k [NO] 2 NO(g)--> N₂O₂(9) N₂O₂(g) + O₂(9) --> 2 NO₂(9) Ratek [NO]2 [0₂11/2
5*) a) The reaction A B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of [A] of 0.100 M. What is the initial rate at [A]o = 0.500 M? b) The reaction below was experimentally determined to be first order with respect to O2 and second order with respect to NO. O2(g) + 2 NO(g) → 2 NO2(g) The diagrams provided represent reaction mixtures in which the number of each type of molecule represents its relative initial concentration. Which mixture has the fastest initial rate? Explain. KEY: = 02 = NO (i) (ii) (iii)
7. For the decomposition of (CH3)20 (species A) at 777 K, the time required for [A], to fall to 0.69[A], as a function of [A], is: 8.13 6.44 3.10 10 [A], (mol · dm-3) | to.69 (S) 1.88 590 665 900 1140 (a) Determine the order of the reaction graphically. (Give the final answer to one decimal place.) (b) Determine the value of ka (include appropriate units) in = -kĄ[A]". Show detailed d[A] dt workings. (Give the final answer to three significant figures in scientific notation.)
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F2 + CIO,→FC102 + F step 2 fast: F+ ClO2 → FCio, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]"[B]"... , where 'l' is understood (so don't write it) for m, n etc.) Rate =
For a type II second-order reaction, the reaction is 60% complete in 60 seconds when [A]0 =0.1 M and [B]0 = 0.5 M.a) What is the rate constant for this reaction?b) Will the time for the reaction to reach 60% completion change if the initial reactantconcentrations are decreased by a factor of two?