Task-2: The importance of heterogeneous catalysis in modern life is evidenced by the fact that numerous products and technologies routinely used nowadays involve catalysts in their synthesis or function. The discovery of catalytic materials is, however, a non-trivial procedure, requiring tedious trial-and-error experimentation. A generalized treatment of heterogeneous chemical reactions is developed and applied to several sublimation, catalytic, and oxidation processes. Based on this concept illustrate the following concepts with key industrial applications. i) Heterogeneous reacting systems

Task-2: The importance of heterogeneous catalysis in modern life is evidenced by the fact that numerous products and technologies routinely used nowadays involve catalysts in their synthesis or function. The discovery of catalytic materials is, however, a non-trivial procedure, requiring tedious trial-and-error experimentation. A generalized treatment of heterogeneous chemical reactions is developed and applied to several sublimation, catalytic, and oxidation processes. Based on this concept illustrate the following concepts with key industrial applications. i) Heterogeneous reacting systems

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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For an autocatalytic reaction : A → B + …… where -d[A]/dt = k[A][B]. Assume that [B]o ≠0 Letting [A] = Ao – x and [B] = Bo +x -d[A]/dt = -d[Ao -x]/dt = dx/dt and dx/dt = k[Ao- x] [Bo + x] Show that [B] = {[A]o + [B]o } / [Ao/Bo] exp{- [A]o + [B]0 }kt + 1
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Question: What is the fundamental difference between kinetic stability and thermodynamic stability in chemical reactions, and how do they influence reaction rates?
10. The rate of change in colour of iodide (yellow) can be measured as it reacts with colourless hypochlorite, OCI (ag): I (aq) + OCI(aq) I0- (aq) + Cl (aq) a. Different concentrations of reactants are combined at the same temperature and the rate of yellow colour disappearance were measured: Rate of colour Trial Initial [I] (mol/L) Initial [OCI(ag)) change (mol/(L s) 0.12 0.18 7.91 x 102 1 0.18 3.95 x 102 0.060 0.090 0.030 9.88 x 103 3 0.24 7.91 x 102 4 0.090 Using the data provided, calculate the value of the rate constant, including units b. Predict the rate of reaction if both reactants have an equal starting concentration of 0.10 mol/1.
What are the main experimental techniques used to characterize catalysts in terms of: (i) chemical composition; (ii) structure; (iii) acidic or basic properties; (iv) texture; (v) morphology.
11:27 2NH4+ (aq) + HCO3- (aq) The reaction is first order with respect to urea, and first order overall with a rate constant of 4.28 x 10^(-4)s^(-1) a. Write the rate law for this reaction. b. If the reaction begins with an initial urea concentration of 0.500 M, what will the concentration of urea in the solution be after 2500 s? C) Calculate the half life of this reaction. d. At what time (+) will the concentration of urea be 0.020 M? O □
Knowledge about the speed of chemical reactions is extremely important for industrial production, especially when optimizing a process. In this sense, strategies can be developed based on changes in the surface area, concentration of reactants, system temperature, and the use of catalysts. Considering this information, analyze the following statements: I. The frequency and orientation of collisions between the reacting species, as well as the amount of energy in the system, are determining factors for the formation of the activated complex. II. The use of catalysts provides an alternative pathway for the formation of the activated complex with lower activation energy, consequently increasing the reaction rate. III. Exothermic transformations are more advantageous because they release energy during product formation, thereby eliminating the need to supply energy to the reactants. Is it correct to assert that:
Consider the reaction data. A products T (K) | k (s-1) 325 0.383 825 0.611 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. X1 Yi = X2 = Y2 = Determine the rise, run, and slope of the line formed by these points. rise: run: slope: What is the activation energy of this reaction? Ea J/mol ? II
True or False: 1. The initial concentration of an intermediate is assumed as 0 when using steady-state approximation. 2. A spontaneous reaction with ΔG = -1070 J/mol happens at 562 K, the Keq of this process is less than 1.
Regarding the activated complex, it can be stated that: (I) Its existence is fleeting, as long as the reaction takes place, but it disappears when it ends. (II) It is easily observable in any reaction. (III) It has the same properties as a reaction intermediate. (IV) It is simply the point of maximum energy in the corresponding reaction energy profile.
to access important values if needed for this question. For the gas phase decomposition of ethyl chloroformate, CICOOC₂H5 C₂H5Cl + CO₂ the rate constant in s¹ has been determined at several temperatures. When Ink is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -1.48 x 104 K and a y-intercept of 24.6. The value of the rate constant for the gas phase decomposition of ethyl chloroformate at 465 K is s-1
6. To observe the effect of temperature on reaction rate, the reaction between MnO, ag) and C204(ag) in acidic media is performed according to the given redox reaction: 2 MnO4 (aq) + 16 H*(aq) + 5 C204²(aq) → 10 CO2(g) + 2 Mn²"(aq) + 8 H2O(1) At various temperatures, the rate constants were determined experimentally as follows: k (M s') 5.03x105 T (°C) 20 35 3.68×104 60 6.71×103 90 0.119 (a) Determine Ea for this reaction by a graphical method (see the graph given below). (b) Determine E. using Arrhenius equation using tabulated data. (c) Calculate the value of the rate constant, k at 100°C. -2 -4 兰 -6 -8 -10 -12 0.0025 0.0027 0.0029 0.0031 0.0033 0,0035 1/T (K)