SOLVE AND EXPLAIN STEP BY STEP The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:AsO 3³ +2 Ce4+ + H₂O →→→ AsO4³- + 2 Ce³+ + 2 H+Experiment [As03³¯] M[Ce4+], MInitial Rate, Ms¯¹2.42×10-2 0.24212344.84x10-2Rate =2.42×10 24.84x10-20.242From these data, the rate constant is0.4850.4857.11x10-41.42x10-32.86x10-3Complete the rate law for this reaction in the box below.Use the form K[A][B]". If m or n are 1, don't enter the 1. Omit concentrations taken to the zero power.5.72x10-3M-25-1.

Answered: Image /qna-images/answer/b8ebab13-2953-40fc-8256-65677cc130e5.jpg

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO3³ +2 Ce4+ + H₂O → AsO₂³+2 Ce³+ + 2 H+ Experiment [AsO 3³ ]o, M [Ce4+] or M Initial Rate, Ms™¹ 1 2 3 4 2.42×10-2 Rate = 4.84x10-2 2.42x10-2 4.84x10-2 0.242 From these data, the rate constant is 0.242 0.485 0.485 7.11x10-4 1.42x10-3 2.86x10-3 Complete the rate law for this reaction in the box below. Use the form K[A][B]". If mor n are 1, don't enter the 1. Omit concentrations taken to the zero power. 5.72x10-3 M-25-1.

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO3³ +2 Ce4+ + H₂O → AsO₂³+2 Ce³+ + 2 H+ Experiment [AsO 3³ ]o, M [Ce4+] or M Initial Rate, Ms™¹ 1 2 3 4 2.42×10-2 Rate = 4.84x10-2 2.42x10-2 4.84x10-2 0.242 From these data, the rate constant is 0.242 0.485 0.485 7.11x10-4 1.42x10-3 2.86x10-3 Complete the rate law for this reaction in the box below. Use the form K[A][B]". If mor n are 1, don't enter the 1. Omit concentrations taken to the zero power. 5.72x10-3 M-25-1.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 25QRT

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