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The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2+ 2UO₂+ + 4H+ → U¹+ + UO₂²+ + 2H₂O Experiment [UO₂+], M [H+]o, M Initial Rate, M.s¯¹ 0' S 0.00458 0.714 0.00238 0.00916 0.714 0.00953 0.00458 1.43 0.00477 0.00916 1.43 0.0191 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 1 2 3 4 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M-2 S-1

The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2+ 2UO₂+ + 4H+ → U¹+ + UO₂²+ + 2H₂O Experiment [UO₂+], M [H+]o, M Initial Rate, M.s¯¹ 0' S 0.00458 0.714 0.00238 0.00916 0.714 0.00953 0.00458 1.43 0.00477 0.00916 1.43 0.0191 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 1 2 3 4 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M-2 S-1

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 57AP
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The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2+ 2UO₂+ + 4H+ → U4+ + UO₂²+ + 2H₂O + Experiment [UO₂+]o, M [H]o, M Initial Rate, M. s-¹ 0.00458 0.714 0.00238 0.00916 0.714 0.00953 0.00458 1.43 0.00477 0.00916 1.43 0.0191 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 1 2 3 4 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M-² • S -1
Transcribed Image Text:The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2+ 2UO₂+ + 4H+ → U4+ + UO₂²+ + 2H₂O + Experiment [UO₂+]o, M [H]o, M Initial Rate, M. s-¹ 0.00458 0.714 0.00238 0.00916 0.714 0.00953 0.00458 1.43 0.00477 0.00916 1.43 0.0191 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 1 2 3 4 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M-² • S -1
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