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 ← Adsorption of B: B+S₂ A. S₁ B-S2 Surface reaction: A S₁+B S2C+S₁ + S₂ KA, KA KB, KB krxn where k and K represent 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 ← Adsorption of B: B+S₂ A. S₁ B-S2 Surface reaction: A S₁+B S2C+S₁ + S₂ KA, KA KB, KB krxn where k and K represent 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 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?
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.
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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(b) The reaction between H2O2 and lodide; H,0, + 21 + 2H*→ 2H,0 + 12 Proceeds by two parallel mechanism and led to a rate laws, k, [H,0][I] and = k, [H,0][][#*] %3D dt dt The change in observed rate constants with ionic strength for both the mechanisms is given in the following table. k (M's) 0.69 k2 (M's') Sr. no. Ionic strength (1) 19.0 0.00 0.0207 0.66 15.0 3 0.0525 0.67 12.0 4 0.0925 0.68 11.3 0.69 0.1575 0.2025 9.7 0.71 9.2 With the help of this data and corresponding plots, comment on which mechanism between these two would follow Primary salt effect more prominently. rhich tyne of complex mechanism T-jump
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Briefly explain the techniques of catalyst characterization: c) FT-IR of solids with pyridine adsorbed) XRD in the analysis of a catalyst
4. a. (i) The maximum kinetic isotope effects (KIE) are exhibited for the reactions of molecules which involve the isotopes of hydrogen. By outlining the origins of KIE, explain why this is so. (ii) Present an expression which gives the dependence of the rate constant k on H/D isotopic substitution i.e., predict kµ / kp.
2. Czarnowski and H.J. Schuhmacher (Chem. Phys. Lett. 17, 235 (1972)) suggested the following mechanism for the thermal decomposition of F2O in the reaction 2 F20(g) → 2 F2(g) + O2(g): 1) F2O+ F2O →F+OF + F2O : ka ko ke kd 2) F+F20 → F2 + OF: 3) OF + OF → 02 + F + F : 4) F+F+ F2O→ F2 + F2O: Use the steady-state approximation to find the rate law of this reaction.
P17D.4 The second- order rate constants for the reaction of oxygen atoms with aromatic hydrocarbons have been measured (R. Atkinson and J.N. Pitts, J. Phys. Chem. 79, 295 (1975)). In the reaction with benzene the rate constants are 1.44 x 10 dm3 mol s at 300.3 K, 3.03 x 10 dm mol s at 341.2 K, and 6.9 x 10 dm3 mols at 392.2K. Find the frequency factor and activation energy of the reaction.