B. A reaction (A + B → C) was catalyzed by a solid catalyst with dual surface sites (S1 and S2) via a reaction mechanism proposed in below: Adsorption of A: A+S₁ A S₁ Adsorption of B: B+S2B S₂ Surface reaction: A S₁+B S2C+S₁ + S₂ KA, KA KB, KB A Krxn where k and K représent forward rate constant and equilibrium constant, respectively. Assuming the surface reaction is the rate-determining step, derive the expression for the formation rate of C.

B. A reaction (A + B → C) was catalyzed by a solid catalyst with dual surface sites (S1 and S2) via a reaction mechanism proposed in below: Adsorption of A: A+S₁ A S₁ Adsorption of B: B+S2B S₂ Surface reaction: A S₁+B S2C+S₁ + S₂ KA, KA KB, KB A Krxn where k and K représent forward rate constant and equilibrium constant, respectively. Assuming the surface reaction is the rate-determining step, derive the expression for the formation rate of C.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

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The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
9. The following shows 3 step reaction mechanism of decomposition reaction of N₂Os: T Step 1: ka,ka. N₂O5 NO₂ + NO3 sili od bluow Jadw .sbflluzib (ka for the forward reaction a noitushogs Step 2: to fom (NO₂ + NO3 mobilusis Step 3: hilleil, NO + N₂O. N₂05→ Using steady-state approximation, deduce the decomposition rate of N₂O5. dX=TA ction and ka' for the reverse reaction) ka for the reverse reaction to g 00.211 NO₂+ O₂ + NOO Saoitoloe aid) lo imioq gailiod NO₂ + NO₂ + Nouillod to 256 bus (garA) NO₂ (q 01)
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NH3 is used as an agent for NO reduction in the temperature range of about 1,000 K. The mechanism for NO reduction by NH; contains the following reaction steps: NH3 + OH NH2 + H2O (RI) NH2 + NO – N2 + H+ OH (R2) NH, + NO – N, + H,O (R3) H+02 -0+ OH (R4) O+ H2O → OH+ OH (R5) Show that the above process runs away when the (branching) ratio of the rate of the branching reaction (R2) over that of the termination reaction (R3) exceeds the critical value of 1/3. Assume that NH2, H, and O are in steady state.
(1) The gas phase decomposition of dinitrogen pentoxide at 335 KN2O5(g)2 NO2(g) + ½ O2(g)is first order in N2O5 with a rate constant of 4.70×10-3 s-1.If the initial concentration of N2O5 is 3.97×10-2 M, the concentration of N2O5 will be 8.22×10-3 M after ______s have passed. (1b) The gas phase decomposition of sulfuryl chloride at 600 K SO2Cl2(g) SO2(g) + Cl2(g) is first order in SO2Cl2 with a rate constant of 2.80×10-3 min-1. If the initial concentration of SO2Cl2 is 4.90×10-3 M, the concentration of SO2Cl2 will be M after ______ 499 min have passed.
Briefly explain the techniques of catalyst characterization: c) FT-IR of solids with pyridine adsorbed) XRD in the analysis of a catalyst
E17D.4(b) The activation energy for the decomposition ofbenzene diazonium chloride is 99.1 kJ mol". At what temperature is the rate constant 10 per cent greater than at 25 °C? 16