-Tabulated below are initial rate data for the reaction:2 Fe(CN),- + 2E→ 2Fe(CN),4- + l2Run [Fe(CN),3-(M)(Fe(CN),J.(M)Initial Rate(M)(M)(M/s)0.010.010.010.020.020.020.020.010.010.010.020.020.010.010.010.011 x 10-52x 10-58x 10-58x 10-58x 10-50.020.020.02What is the value of k?12345

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-Tabulated below are initial rate data for the reaction: 2 Fe(CN),- + 2E 2Fe(CN),4- + l2 Run [Fe(CN),-b (M) (Fe(CN)6l (M) [l2]o (M) Initial Rate (M) (M/s) 0.01 0.01 0.02 4 0.02 1 0.01 0.02 0.02 0.02 0.02 0.01 0.01 0.01 0.02 0.02 0.01 0.01 0.01 0.01 0.02 1x 10-5 2x 10-5 2 3 8x 10-5 8x 10-5 8x 10-5 5 0.02 What is the value of k?

-Tabulated below are initial rate data for the reaction: 2 Fe(CN),- + 2E 2Fe(CN),4- + l2 Run [Fe(CN),-b (M) (Fe(CN)6l (M) [l2]o (M) Initial Rate (M) (M/s) 0.01 0.01 0.02 4 0.02 1 0.01 0.02 0.02 0.02 0.02 0.01 0.01 0.01 0.02 0.02 0.01 0.01 0.01 0.01 0.02 1x 10-5 2x 10-5 2 3 8x 10-5 8x 10-5 8x 10-5 5 0.02 What is the value of k?

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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Rate = k[HOOBr][HBr] Rate = k[HBr][O21 QUESTION 6 The following questions are based on the reaction and data below. Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution this reaction takes place: 2CIO 2(aq) + 20H (aq) → CIO 2 (aq) + CIO 3 (aq) + H2O(). Based on the following data, determine the rate law and the value of the rate constant. Initial Concentrations Initial Rate [CIO2] [OH] (M/s 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 What is the order of the reaction with respect to HO? Second order First order Zero order O Fourth order QUESTION 7
R=K [A] [B] ----; 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] 1 0.10 0.10 0.10 2 0.20 0.10 0.10 3 0.10 0.20 0.10 4 0.10 0.10 0.20 A) Determine the rate law equation including the k value. Determine the order of reaction for BrO3, Br, and H* Rate law 3 Br₂(l) + H₂O(l) Initial rate (mol/Ls) 8.0 x 104 1.6 x 10³ 1.6 x 10°³ 3.2 x 10'³
Consider the following reaction and information: A + 2B → 3C rate = k{B} Time (min.) B (M) A (M)0 0.72 0.5030 0.25 0.2660 0.087 0.18 What is the concentration of B after 27 minutes?
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3- The initial-rate method was applied to the decomposition of nitrogen dioxide, 2NO2(g) --> 2No(g) + O2(g) Initial concentration of NO2 Initial rate of formation of O2 1- 0.010mol/L 7.1X10-5 mol(L.s) 2- 0.020mol/L 28.5X10-5 mol(L.s) Find the rate law and the value of the rate constant with respect to O2 formation?
Need the following questions answered The reaction of interest: NO2 (g) + CO (g) → NO + CO2 (g) Expt. [NO2] (M) [CO] (M) Initial Rate (M/s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the reaction order for nitrogen dioxide? What is the reaction order for carbon monoxide? What is the overall reaction order? What is the rate law for this reaction? What is the specific rate constant (k) for this reaction? Write the rate law for this reaction that includes the numerical value of the specific rate constant:
Question 40 of 49 Find the value of k for the rate law: Where the rate = 4.0*x 10-³ M/s, NO=0.45M and H+=1.15M A) 0.000932 1/M²s B) 0.00773 1/M²s C) 0.00207 1/M²s D) 0.0172 1/M²s rate = k [NO]²[H+*]⁰ E) 0.0198 1/M²s
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91. For the reaction 2N,Os (9) + 4NO, (g) + O2 (g) the following data were collected, where A [N2O5] Rate At Time (s) T- 338 K (N2Os] T= 318 K (N2O,] 1.00 x 10- M 1.00 x 10-1 M 100. 6.14 x 10- M 9.54 x 10- M 300. 2.33 x 10- M 8.63 x 10- M 600. 5.41 x 10 M 7.43 x 10- M 1.26 x 10 M 6.39 x 10- M 900. Calculate E, for this reaction.
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The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and I2(g) is given here. What is the activation energy for the reaction? 2HI(g) ⟶ H2(g) + I2(g)