The following initial rate data were found for the reaction:\[ 2\text{MnO}_4^- + 5\text{H}_2\text{C}_2\text{O}_4 + 6\text{H}^+ \rightarrow 2\text{Mn}^{2+} + 10\text{CO}_2 \]| Experiment | [MnO₄⁻] (M) | [I⁻] (M) | [H⁺] (M) | Rate (M/s) ||------------|------------|----------|----------|-------------|| 1 | 1.00×10⁻³ | 1.00×10⁻³ | 1.0 | 2.0×10⁻⁴ || 2 | 2.00×10⁻³ | 1.00×10⁻³ | 1.0 | 8.0×10⁻⁴ || 3 | 2.00×10⁻³ | 2.00×10⁻³ | 1.0 | 1.6×10⁻³ || 4 | 2.00×10⁻³ | 2.00×10⁻³ | 2.0 | 1.6×10⁻³ |The rate law for this reaction is:- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄][H⁺]- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]⁵[H⁺]⁶- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]- ⊗ Rate = k[MnO₄⁻][H₂C₂O₄][H⁺]- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]²This data can be used to determine the appropriate rate law expression for this chemical reaction based on the influence of different initial concentrations on the reaction rate.

Answered: Image /qna-images/answer/adc4be09-1952-48e1-8556-678282f3da7f.jpg

The following initial rate data were found for the reaction 2MnO4 + 5H2C2O4 + 6H+ → 2 Mn²+ [MnO4-] (M) 1.00×10-3 2.00×10-3 2.00×10-3 2.00×10-3 The rate law for this reaction is Experiment 1 2 3 4 Rate = K[MnO4]2[H₂C₂O4][H+] Rate = k[MnO4]2[H₂C₂O4]5[H+]6 Rate = k[MnO4]2[H₂C₂O4] Rate = k[MnO4][H₂C2O4][H*] Rate = k[MnO4]²[H₂C₂O4]² [1-] (M) 1.00×10-3 1.00×10-3 2.00×10-3 2.00×10-3 {H+] (M) 1.0 1.0 1.0 2.0 + 10 C Rate (M/s) 2.0×10-4 8.0×10-4 1.6×10-3 1.6×10-3

The following initial rate data were found for the reaction 2MnO4 + 5H2C2O4 + 6H+ → 2 Mn²+ [MnO4-] (M) 1.00×10-3 2.00×10-3 2.00×10-3 2.00×10-3 The rate law for this reaction is Experiment 1 2 3 4 Rate = K[MnO4]2[H₂C₂O4][H+] Rate = k[MnO4]2[H₂C₂O4]5[H+]6 Rate = k[MnO4]2[H₂C₂O4] Rate = k[MnO4][H₂C2O4][H*] Rate = k[MnO4]²[H₂C₂O4]² [1-] (M) 1.00×10-3 1.00×10-3 2.00×10-3 2.00×10-3 {H+] (M) 1.0 1.0 1.0 2.0 + 10 C Rate (M/s) 2.0×10-4 8.0×10-4 1.6×10-3 1.6×10-3

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...

See similar textbooks

Similar questions

A reacts with B according to the equation: 2 A + B → A₂B The data below were collected for this reaction. Trial 1 Trail 2 k= Trial 3 Determine the rate law. Calculate the value for k. What are the correct units for k? [A]initial (M) 4.50×10-² 4.50×10-² 9.00×10-2 [B]initial (M) Initial (M s-¹) 1.70×10-3 2.25x10-3 3.40×10-3 9.00×10-3 1.70x10-3 2.25x10-3 7151713
Determine the overall rate law for the reaction CH3Br(aq) + OH (aq) → CH3OH(aq) + Br (aq). The data is given below Experiment [CH3B1] (M) [OH"] (M) Initial rate (M/s) k[CH3B1][OH¯]³ O k[CH3B1]°[OH73 1 0.12 0.12 5.2 x 10-5 O k[CH3B1]?[OH"7² 2 0.24 0.12 1.04 x 10-4 O k 3 0.12 0.06 6.5 x 10-6 O KỊCH3B1]°[OH"]) O k(CH3B1]?[OH"]
Consider the generic reaction below. A + B --> C + D Given the following data and graph, determine the rate law for the reaction. Trial 1 [A] 0.10 M [B] 0.10 M Absorbance (A 1.55- 1.50 1.45- 1.40- 0 Trail 2 0.14 M 0.10 M 0.5 Trial 1 - Trial 2 1.0 Time (s) Trial 3 0.10 M 0.20 M Trial 3 1.5 2.0
Determine the rate law for the data below and give the value of the rate constant (k). If you have the constant correct, the rest of the rate law should also be correct :) Experiment Initial A Initial B Rate of Formation for C 1 0.00036 0.0052 5.3980x10-7 2 0.00036 0.0104 1.0796x10-6 3 0.00018 0.0104 2.6990x10-7
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
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 3+ AsO3³ + 2Ce¹+ + H₂O → AsO4³ + 2Ce³+ + 2H+ Rate = k = [ASO3³] [Ce¹+] M M 0.0311 0.0622 0.0311 0.0622 M-2.s I 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 0.145 0.145 0.290 0.290 Initial Rate, M.s-1 S 0.000345 0.000690 0.00138 0.00276
What is the rate constant for the reaction?
Calculate the rate law from the given data: Run [B] [C] Initial Rate (M/sec) 1 1.5 2.0 0.20 2 1.5 4.0 0.40 3 3.0 2.0 0.80
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.