Use the Rele.to access impevalues if needed for this questionThe following initial rate data are for the reaction of UO,* with hydrogen ion in aqueous solution:2 UO,* + 4 Ht+ U0,* -+ 2 H2O[UO,],, M1.39x10-32.78×103Experiment[H*]o, MInitial Rate, M s-111.35×1040.4500.4505.39x1042.2.70x1041.08×10-331.39x10-30.900142.78x10-30.900Complete 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 isM?s!. The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solutionOCr +I OI + CIis first order in OCI and first order in I.Complete the rate law for this reaction in the box below.Use the form k[A]™[B]"... , where 'l' is understood for m, n ...(don't enter 1) and concentrations taken to the zero power do not appear.Rate =In an experiment to determine the rate law, the rate constant was determined to be 86.4 M's. Using this value for the rate constant, the rate of the reaction when[OCr] = 2.36x10-3 M and [I] = 3.83×10-3 M would be|Msl.

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The following initial rate data are for the reaction of UO,† with hydrogen ion in aqueous solution: 2 UO,+ + 4 H* u* + U0,²* + 2 H2O Experiment [UO,*], M 1.39x10-3 2.78×10-3 1.39x103 2.78×10-3 [H],, M Initial Rate, M s-! 0.450 1.35×104 2 0.450 5.39x104 3 0.900 2.70x104 0.900 1.08×10-3 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 M2s-1

The following initial rate data are for the reaction of UO,† with hydrogen ion in aqueous solution: 2 UO,+ + 4 H* u* + U0,²* + 2 H2O Experiment [UO,*], M 1.39x10-3 2.78×10-3 1.39x103 2.78×10-3 [H],, M Initial Rate, M s-! 0.450 1.35×104 2 0.450 5.39x104 3 0.900 2.70x104 0.900 1.08×10-3 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 M2s-1

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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The reaction between bromate ions and bromide ions in acidic aqueous solution is given by the following equation: BrO3- (aq) + 5Br- (aq) + 6H+ (aq) --> 3Br2 (l) + 3H2O (l) The experimental results are given below. Experiment Initial [BrO3-] Initial [Br-] Initial [H+] Initial Rate (M s-1) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 Using these data, determine the orders for all reactants, the overall reaction order, and the value of the rate constant.
Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO2+ with hydrogen ion in aqueous solution: 2UO2+4HU++ UO22++ 2H2O Experiment [UO2] M [H] M Initial Rate, M. s¹ 0' 1 0.000748 0.664 0.0000628 2 0.00150 0.664 0.000252 3 0.000748 1.33 0.000126 4 0.00150 1.33 0.000506 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for mor n and concentrations taken to the zero power do not appear. Don't enter 1 for mor n. Rate= k= M-2 -1 S Submit Answer Retry Entire Group 1 more group attempt remaining