EX2Given reaction 4A = B, which has time-independent stoichiometry and kineticequation r = k[A]".When 20% of reactant A is consumed, then the consumption rate ofd[A]A (-=dt= k₁[A]") is measured to be equal to 4×10-³ mol dm-³ s-¹, while when80% of reactant A is consumed, then the consumption rate of A is measured equal to2.5×104 mol dm-³ s-¹.Find the order of the reaction.

Given that 4A→ B-dAdt=kAnlet initial concentration of A be Aowhen 20% A is consumed than…

Answered: EX2 Given reaction 4A = B, which has…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Write -rA solely as a function of conversion (i.e., evaluating all symbols) when the reaction is an elementary, reversible, gas-phase, isothermal reaction with no pressure drop with an equal molar feed and with CA0 = 2.0 mol/dm3, kA= 2 dm6/mol2•s, and KC = 0.5 all in proper units-rA = ____.(e) What is the equilibrium conversion?(f) What is the rate when the conversion is(1) 0%?(2) 50%?(3) 0.99 Xe?
The reaction of CO(g) with NO2 (9) is second-order in NO2 and zero-order in CO at temperatures less than 500 K. a. Write the rate law for the reaction. (Rate expressions take the general form: rate = k[H2][C12].) rate b. How will the reaction rate change if the NO2 concentration is tripled? The reaction rate will be the original value. c. How will the reaction rate change if the concentration of CO is tripled? The reaction rate will be the original value.
s.) 7) The elementary reaction A+B → D is to be carried out to obtain a desired product (D). The rate constant for this reaction is k₁ = 150*exp(-5,000/T). Unfortunately, under conditions required for the reaction to occur, species B also undergoes a second-order decomposition to form an undesired product, B2U, with ry = k₂C, and k₂ = 300*exp(-2,000/T). 212 - a) What is the instantaneous selectivity for this system (SD/U)? Your answer must be simplified as much as possible. 4 Species: A, B, C, D, U YD = rD -VA ŶD= FD KD CA KU FAO-FA 4-02 b) Describe a reactor system (draw a schematic AND describe with words) and operating conditions you would use to maximize the selectivity to D.
QUESTION 8 Regarding the following reaction CO2 (g)+H2 (g)→→CO(g)+H₂O (g) ArH=-41.2kJ/mol Using Le Chatelier's principle to predict (a) to which direction the equilibrium shifts when pressure is decreased. Enter R for reactants, P for products and N for Neither: Direction= ; (b) to which direction the equilibrium shifts when temperature is reduced. Enter R for reactants, P for products and N for Neither: Direction=
For the following reaction 6 experiments have been run and the data collected is in the following table: 2 MnO4-(aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ---> 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l) Experiment [MnO4-], M [H2C2O4], M [H+], M Rate, M/s 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 5 0.4140 0.5740 0.5610 0.3258 6 0.3260 0.4930 0.4910 0.2203 a) Write the rate expression. _____________ b) Calculate the rate constant, k. __________________ c) If the concentration of MnO4-,H2C2O4, & H+ are 0.155 M, 0.293M, and 0.475M respectively, what is the rate of the reaction? ____________________
3.1. Consider the following reaction sequence: k3 S+E = (ES), (ES), → P+E k2 k4 Develop a suitable rate expression for production formation [v = k;(ES)2] by using (a) the equilibrium approach, and (b) the quasi-steady-state approach.
QUESTION 2 Regarding the following reaction at 298.15 K: 4 HCI (g) + O2 (g) →→ 2Cl₂ (g) + 2H₂O (1) The following table lists the stand enthalpy of formation, the standard entropy and the standard formation Gibbs energies Cl2 (g) O2 (g) 0 H₂O (1) -285.83 0 HCI (g) -92.31 186.91 -95.3 69.91 4+Ho(kJmol-1) sº (JK-1mol-1) 4Gº (kJmol-1) 205.14 0 223.07 0 ? Please calculate the standard reaction entropy 4,S°(JK-1mol-1), the standard reaction enthalpy Hº(kJmol-1), the standard reaction Gibbs energy 4,Gº(kJmol-1), and the maximum nonexpansion work that can be gained from the oxidation of HCI (g) at 298.15K. Instruction: Please enter all answers with two decimal places, for example: -344.101 is written as -344.10, please pay attention to the units, particularly As in J/(K.mol) while others is kJ/mol (1) 4,5°(JK-1 mol-1) = (2) 4,H°(kJmol-1) = Please using your results from (1) and (2) to calculate the the standard reaction Gibbs energy:
The value of ArxnH° is 12.93 kJ/mol at 850 K for H₂ (g) + 12 (g) = 2 HI(g) (a) Assuming that ArxnH° is independent of temperature, compute Kp at 700 K given that it is 29.1 at 1000 K. (b) Under this same assumption (constant ArxnHᵒ), at what temperature would you predict that the equilibrium constant for this reaction would have the value Kp = 20?
13.86. The rate constant for the reaction NO₂(g) + O3(g) → NO3(g) + O₂(g) was determined over a temperature range of 40 K, with the following results: T (K) 203 213 223 233 243 k (M¹s¹) 4.14 X 105 7.30 X 105 1.22 X 106 1.96 X 106 3.02 X 106 a. Determine the activation energy for the reaction. b. Calculate the rate constant of the reaction at 300 K.
For the following reaction set, define or propose two types of reactor systems to maximize product D selectivity, sketch the reactor system and describe clearly the input reactant concentrations and separation requirements if necessary. The unit of reaction rate is in units (mol/dm^3.sec) and concentration in units (mol/dm^3). (question on picture)
You are carrying out a reaction in the laboratory. You need to convert 1.00 mole of reactant X into products. This reaction shows first-order kinetics, and the reaction mixture has a constant volume of 1.00 L. At 1:00pm, you start the reaction at 25\deg C with 1.00 mole of reactant X. At 2:00pm, you find that 0.70 moles of reactant X remain. You immediately increase the temperature of the reaction mixture to 35\deg C. At 3:00pm, you discover that 0.25 moles of reactant X are still present. You want to be able to finish the reaction by 4:00pm, but you cannot stop the reaction until only 0.01 moles of reactant X remain. You must increase the temperature again. What is the minimum temperature required to complete the reaction by 4:00pm? (Remember, the reaction is complete when only 0.01 moles of X remain.)
give handwritten answer-A+B -> X (kx) A+B -> Y (ky) A+B -> Z (kz) The substances A and B (with the initial concentration CA0=3 M and CB0=1 M) react in parallel (competing) reactions. What are the individual rate constants (kx,ky,kz) knowing that at the end of the reaction the proportions of the X,Y,Z are 8%, 91%, 1%, and after the first half hour the concentration of A becomes 2.2 M. The answer should be: kx = 1.73 x 10^(-3) L/mol*s ky = 1.97 x 10^(-2) L/mol*s kz = 2.17 x 10^(-4) L/mol*s

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