Given a reaction that occurs through the collision of A and B. Calculate the rate law, and showwhen it behaves as a diffusion-controlled reaction.(- k,' + A + B{l -k+А + в -k, — АВP

A chemical reaction happens when the two or more substrates are combined together to form an…

Answered: Given a reaction that occurs through…

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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2. At 325°C, N0,(g) reacts with CO(g) to yield NO(g) and CO,(g). The reaction is: NO,(g) + CO(g) I NO(g) + CO,(g) It is observed that the reaction rate does not depend upon the concentration of CO, and t\so the reaction rate law does not involve [CO]. The rate does depend upon [NO,], however, and the following data is obtained. Determine the rate law and the value of the rate constant. Rate ( M sec ') NO,] 1. 1 X 10 -2 0.15 4.5 X 10-2 0.3 1.8 X 10- 4.0 X 10-13 0.6 0.9
At a particular time for the reaction Br₂ + 3Cl₂ --> 2BrCl3, the rate of disappearance of Cl₂ was 0.450 mol L¹ s¹. The rate of appearance of BrCl3 at this time can be calculated to be O 0.675 mol L-¹ s¹¹. O 0.900 mol L-¹s1. O 0.300 mol L-¹s¹. O 0.150 mol L ¹1.
1 of 1 Assignment 3 (NCHE312) The total pressure of the following system is used to monitor the progress of the chemical reaction. SO₂Cl₂(g) → SO2(g) + Cl₂(g) The reaction is initiated, and the following data are obtained: Time (h) PTotal (kPa) Pso₂cl₂ Ps0₂ Pclz 0 11.07 3 6 14.79 17.26 9 18.90 12 19.99 15 20.71 Additional information: As the reaction proceeds, stoichiometry dictates that for every mole of SO₂Cl₂ that dissociates one mole of each of SO₂ and Cl₂ is produced. Defining the extent of dissociation/reaction as E, and the initial pressure as Po, the total pressure is given by: Ptotal = Pso₂Cl₂ + Pso₂+ Pcl₂ = (Po-5)+5+5 Convert your work into a single PDF file and upload it into your eFundi Dropbox folder. Deadline for submission: 26/05/2023 at 12pm a) Calculate the pressure of each component at each time interval, i.e. complete the above table. b) Use a graphical method and determine what the order of the reaction is with respect to SO₂Cl₂? (i) Show the plot as well as the…
The decomposition of an organic molecule with the formula C4H6 at 326°C is measured as the decrease of C4H6: Calculate the rate constant for the reaction.
Consider the following reaction mechanism: Step 1: 2NO (g) + 1.50,(g) --> N,Og(s) Step 2: 2NO,(g) --> 2NO(g) + O2 (g) Write the overall reaction and identify any reaction intermediates.
For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
2) For a first order reaction the concentration of the reactant A changes with time according to the following table: t(s) [A] (M) 0 0.110 200 0.073 400 0.048 600 0.032 1000 0.014 A) Find the rate constant k graphically? Prove your answer mathematically? B) Find the concentration of A at 100 s graphically? Prove your answer mathematically?
Consider the following 2-step reaction mechanism, consisting of elementary steps: k1 2 XO2g) k-1 Step 1: X2O4(g) k2 Step 2: X2O4(g) + Br2७) Br2(g) + 2 XO2Br(g) a) Complete the following (if none exist, write 'none'). The reaction intermediate(s) is/are... i) The reaction catalysts(s) is/are.. b) Without assuming the relative reaction rates of Step 1 or Step 2, determine the rate law that is predicted by this mechanism. If Step 2 is a fast reaction (and Step 1 was a slow equilibrium), determine the overall reaction order.
Consider this overall reaction, which is experimentally observed to be second order in X and first order in Y: X + Y -----> XY Does the reaction occur in a single step in which X and Y collide and is the two-step mechanism (below) valid?
The following mechanism has been suggested for a reaction: NO(g) + Br2(g) → NOBR2(g) fast NOBR2(g) + NO(g) 2 NOBr(g) slow (a) What is the overall reaction? (b) What are the intermediates in the mechanism? (c) What is the rate law for the reaction? Edit View Insert Format Tools Table 12pt v Paragraph B IUA IMG F4 F5 F6 E10
Consider this reaction: 2H,PO, (ag) – P,0, (aq)+ 3H,0 (aq) At a certain temperature it obeys this rate law. rate = (0.392 M-1.s Suppose a vessel contains H, PO, at a concentration of 0.520 M. Calculate how long it takes for the concentration of H, PO, to decrease to 12.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
A reaction is identified as zero-order in one of its reactants, X. Time (s) [X] (M) 0 1.50 110 0.80 Based on the data and integrated rate law, what is the rate constant for the reaction at this temperature? k = [?] x 10 M-s-1 coefficient (green) exponent (yellow) Enter

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Given a reaction that occurs through the collision of A and B. Calculate the rate law, and show when it behaves as a diffusion-controlled reaction. (-k' → A + B A + B - k → AB l-k+ P