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The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2UO₂+ + 4H+ → U4++ UO₂2+ + 2H₂O Experiment [UO₂+]o, M [H+], M Initial Rate, M.s¯¹ 0.00181 0.494 0.000254 0.00362 0.494 0.00102 0.00181 0.988 0.000508 0.00362 0.988 0.00203 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. 1 2 3 4 Rate = k= M-2.s-¹

The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2UO₂+ + 4H+ → U4++ UO₂2+ + 2H₂O Experiment [UO₂+]o, M [H+], M Initial Rate, M.s¯¹ 0.00181 0.494 0.000254 0.00362 0.494 0.00102 0.00181 0.988 0.000508 0.00362 0.988 0.00203 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. 1 2 3 4 Rate = k= M-2.s-¹

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.32PAE: 11.32 The following experimental data were obtained for the reaction 2A + 3 B—C + 2D [A](mol L 1)...
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The following initial rate data are for the reaction of UO₂+ with hydrogen ion in aqueous solution: 2UO₂+ + 4H+ → U4++ UO2²+ + 2H₂O Experiment [UO₂+]o, M [H+], M Initial Rate, M. s¯ 0' 0' 0.00181 0.494 0.000254 0.00362 0.494 0.00102 0.00181 0.988 0.000508 0.00362 0.988 0.00203 1 2 3 4 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 = 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: 2UO₂+ + 4H+ → U4++ UO2²+ + 2H₂O Experiment [UO₂+]o, M [H+], M Initial Rate, M. s¯ 0' 0' 0.00181 0.494 0.000254 0.00362 0.494 0.00102 0.00181 0.988 0.000508 0.00362 0.988 0.00203 1 2 3 4 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 = k= M-2.s-1
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