4. The initial rate of the reaction: BrO4 (aq) + 5 Br (aq) + 8 H(aq)has been measured at the reactant concentrations shown (in mol/L)Experiment[BrO₁][Br] [H]12340.100.200.100.100.10 0.100.10 0.100.20 0.100.10 0.20a) Determine the rate law equationb) Calculate the rate constant (K) (include units).3 Br₂0 + 4H₂OInitial rate (mol/(L´s))8.0 x 1041.6 × 10-³1.6 × 10-³3.2 x 10³

4. The initial rate of the reaction: BrO4 (aq)+ 5 Br +8 H has been measured at the reactant concentrations shown (in mol/L) (aq) 3 Br20) + 4H₂0) (aq) Experiment [BrO4] [Br] [H] Initial rate (mol/(L-s)) 1 0.10 0.10 2 3 4 0.10 0.20 0.10 0.10 0.10 0.10 0.20 0.10 0.10 0.20 a) Determine the rate law equation b) Calculate the rate constant (K) (include units). - 8.0 × 104 1.6 × 10-³ 1.6 × 10³ 3.2 x 10³

4. The initial rate of the reaction: BrO4 (aq)+ 5 Br +8 H has been measured at the reactant concentrations shown (in mol/L) (aq) 3 Br20) + 4H₂0) (aq) Experiment [BrO4] [Br] [H] Initial rate (mol/(L-s)) 1 0.10 0.10 2 3 4 0.10 0.20 0.10 0.10 0.10 0.10 0.20 0.10 0.10 0.20 a) Determine the rate law equation b) Calculate the rate constant (K) (include units). - 8.0 × 104 1.6 × 10-³ 1.6 × 10³ 3.2 x 10³

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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Part A Consider the balanced chemical equation. H2O2(aq) + 3I¯ (aq) + 2H+(aq) → I3 (aq) + 2H20(1) Predict the rate of change in the concentration of H2O2 (A[H2O2]/At). In the first 12.0 s of the reaction, the concentration of I drops from 1.000 M to 0.773 M . Express the rate to three significant figures and include the appropriate units. You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. ? A[H2O2]/At = Value Units