[References]Use the References to access important values if needed for this question.The following initial rate data are for the reaction of UO, with hydrogen ion in aqueous solution:4+2 UO, + 4 H-U* +U0,2* + 2 H20Experiment[UO,], M[H*],, MInitial Rate, M s14.15x1030.3449.66×104218.30x10-30.3443.86x1034.15x1030.6881.93x103148.30x1030.6887.73x103Complete 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 isM21Submit AnswerTry Another Version10 item attempts remainingPreviousNext63°F RainingDELL3.

From given Rate law and Rate constant have been solved below

[References] Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO, with hydrogen ion in aqueous solution: 2 UO, +4 H*-u* + UO,2+ +2 H,0 Experiment [UO,1, M [H'], M Initial Rate, M s 4.15x103 S.30x103 4.15x103 0.344 9.66x104 0.344 3.86x10-3 3 0.688 1.93x103 S.30x10-3 0.688 7.73x10-3 Complete the rate law for this reaction in the box below. Use the form kJA]" 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

[References] Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO, with hydrogen ion in aqueous solution: 2 UO, +4 H-u + UO,2+ +2 H,0 Experiment [UO,1, M [H'], M Initial Rate, M s 4.15x103 S.30x103 4.15x103 0.344 9.66x104 0.344 3.86x10-3 3 0.688 1.93x103 S.30x10-3 0.688 7.73x10-3 Complete the rate law for this reaction in the box below. Use the form kJA]" 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

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 following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + Hz I, + 2 HCI Experiment [ICI], M [Ha]o, M Initial Rate, M s-1 1.58×10-2 3.16x10-2 6.29x10-2 0.126 1 0.254 0.188 2 0.508 0.188 3 l0.254 0.375 4 0.508 0.375 Complete the rate law for this reaction in the box below, Use the form k[A]"[B]", where '1' is understood for m orn 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
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T[C] K [ cm³/mol-s] The rxn is a decomposition reaction of HI. 2HI → H₂ + 1₂ In this rxn, the ff data were gathered. 508 1.059x10-1 427 3.1x10-3 393 5.88x10-4 356 8.09x10-5 Solve for the complete rate eq. for this reaction [ i.e. r = f(T) f(C) ] 283 9.42x10-7
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* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit
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The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + Hz Iz + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, Ms 1 0.205 6.75x102 1.77x103 0.410 6.75x102 3.53x103 2. 3 0.205 0.135 7.06x10-3 0.410 0.135 1.41×10 2 4 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or Rate = Common Greek(upper) Greek(lower) Arrows Other From these data, the rate constant is X, Ox Aa (s) (1) (g) (aq)
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