The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:As033- + 2 Ce4+ + H20→AS043- + 2 Ce3+ + 2 H+Experiment[As033-]o, M[Ce*+]o, MInitial Rate, M s12.86x10-20.5454.52x10-3125.72x10-20.5459.04x10-332.86x10-21.091.81×10-25.72x10-23.62x10-241.09Complete the rate law for this reaction in the box below.Use the form k[A]™[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.Rate =From these data, the rate constant isM-25-1.

Rate is dependent on the reactants of the reaction. Consider experiment two and experiment one…

Answered: Complete the rate law for this reaction…

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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Q46
Balance the redox reaction K2Cr2O7 + FeSo4 + H2SO4 --> Cr2(SO4)3+ Fe(SO4)3 + K2SO4 + H20
Choose all the statements that is correct A large negative free change for a reaction means that .... A) the reaction greatly favors formation of the products B) only a small amount of product is produced at equilibrium C) the equilibrium constant of the reaction is small D) the equilibrium constant of the reaction is large
REACTION ENGINEERING Consider a heterogeneous gas-phase catalytic reaction:AB(g)→A(g)+B(g) (Catalyst) The surface reaction mechanism follows three steps: AB(g) +S <----> AB*S (Adsorption)AB*S<----> B*S+A(g) (Surface reaction)B*S <---> B(g) + S (Desorption) (a) Derive the rate law assuming (1) surface reaction is rate limiting, and (2) desorption is rate-limiting. Express the overall reaction rate (- Tan) in terms of total number of sites on the surface, C. partial pressures of the gas species (ie., Pab Pa and Pb), rate constants of adsorption, the surface reaction, and desorption (ka,ks, and kd), and the equilibrium constants of adsorption, the surface reaction, and desorption (ie., Ka. Ks and Kd).
Given the following reaction and using the data in the table, determine the order of the reaction:2NO2(g)→2NO(g)+O2(g) Time (sec) [NO2 ] ln [NO2 ] 1/[NO2 ] 0 0.0100 -4.605 100 100 0.00648 -5.039 154 200 0.00479 -5.341 209 300 0.00380 -5.573 263 400 0.00315 -5.760 317 500 0.00269 -5.918 372 600 0.00235 -6.057 426 a. none of these b. second c. zero d. third e. first
For the following reaction, write how each of the indicated changes will affect the indicated amount, assuming a fixed-size reactor. Write "increase", "decrease" or "no change". (Or use an "up" arrow to indicate "increase" and a "down" arrow to indicate "decrease"). (For a chemical added, write how you would respond AFTER the addition.)
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QUESTION 9 Consider the foilowing chemical reaction: X--Y When the reaction data is graphed, the following graphs are produced: In Ex] Lime time [X] time How many minutes will it take for 26.88% of compound X to react?k= 1.25 x 102 (k is measured in seconds)
1. Consider the following unbalanced reaction, Cl2(g) + NO(g) ---> NOCl(g) a). Suppose that 150.0 g of NO is allowed to react with 220.0 g of Cl2. What is the largest amount of NOCl that could be formed in this reaction? b) What was the yield if only 31.5 g was actually formed? (corresponds to part a) 2.Draw a diagram of y against r for a 3s. What 2 features does it imply that do not make much sense? How can these problems be avoided? Give and explanation and diagrams/graphs
1. Houston book, pp. 90, 2.35. Suggest plausible mechanisms for the following two reactions given the overall reaction rate law. a. I- + OCI" CI- + OI-; -d[I]/dr = k[I][OCI"V[OH] %3D b. C(CH,),CI + OH- → C(CH,),OH + CI; -d[C(CH,),CIJ/dr k[C(CH,),CI][OHV{[CI] + K'[OH-]}
for the following reaction [ aA+bB---->product] what does the following terms means: [CA0*XA] ? [CB0*XB] ? what condition which makes the value of XA and XB to be kept constant during all the reaction time ?
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Complete the rate law for this reaction in the box below. Use the form k[A]™[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-251.