4-chemThe following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:AsO3- + 2 Ce** + H,O→ASO,+2 Ce3+ + 2 H*Experiment[AsO3 lo, M[Ce**lo, MInitial Rate, M s-1S11.39x10-20.2414.34x10-42.78×10-20.2418.67x10-431.39×10-20.4821.73x10-3142.78×10-20.4823.47x10-3Complete 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 =From these data, the rate constant isM?s-1.

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4-chem The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO3- + 2 Ce** + H,OASO,- + 2 Ce³* + 2 H* [AsO3 ], M 1.39x10-2 2.78×10-2 Experiment [Ce**], M Initial Rate, M s 1 0.241 4.34x10-4 8.67x10-4 1.73×10-3 2 0.241 3 1.39×10-2 0.482 4 2.78×102 0.482 3.47x10-3 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 = From these data, the rate constant is M?s1.

4-chem The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO3- + 2 Ce** + H,OASO,- + 2 Ce³* + 2 H* [AsO3 ], M 1.39x10-2 2.78×10-2 Experiment [Ce**], M Initial Rate, M s 1 0.241 4.34x10-4 8.67x10-4 1.73×10-3 2 0.241 3 1.39×10-2 0.482 4 2.78×102 0.482 3.47x10-3 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 = From these data, the rate constant is M?s1.

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 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

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The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
You and a coworker have developed a molecule thathas shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law Rate=k[AV]1[V]1 You have been given the following data from your coworker: [V]0=0.20M[AV]0=1.0104M A plot of ln[AV] versus t(s) gives a straight line with a slope of 0.32 s1. What is the value of the rate constant (k) for this reaction?
The rate constant for the ?rst-order decomposition at 45 C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCI3, is 6.2104 min-1. 2N2O54NO2+O2 What is the rate of the reaction when [N2O5] = 0.40 M?
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
Consider a 5.000 M solution of the hypothetical com- pound R. Its decomposition is a second-order reaction and its activation energy is 57.6 kJ/mol. At 759C, the half-life of the 5.000 M solution is 8.49 h. What is the half-life of the same solution at 700C (3 significant figures)?
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:AsO33- + 2 Ce4+ + H2O -------> AsO43- + 2 Ce3+ + 2 H+ Experiment [AsO33-]o, M [Ce4+]o, M Initial Rate, M s-1 1 4.13×10-2 0.463 4.79×10-3 2 8.26×10-2 0.463 9.58×10-3 3 4.13×10-2 0.926 1.92×10-2 4 8.26×10-2 0.926 3.83×10-2 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , 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 = ______From these data, the rate constant is ________ M-2s-1.
The aquation of tris(1, 10-phenanthroline)iron(II) in acid solution takes place according to the equation: Fe(phen)32+ + 3 H3O+ + 3 H2O → Fe(H2O)62+ + 3 phenH+ If the activation energy, Ea, is 126 kJ/mol and the rate constant at 30°C is 9.8 × 10-3 min-1, what is the rate constant at 50°C? Be sure to indicate the correct unit with your answer.
The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution:OCl- + I- OI- + Cl- Experiment [OCl-]o, M [I-]o, M Initial Rate, Ms-1 1 6.78×10-3 4.73×10-3 2.39×10-3 2 6.78×10-3 9.45×10-3 4.77×10-3 3 1.36×10-2 4.73×10-3 4.79×10-3 4 1.36×10-2 9.45×10-3 9.56×10-3 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , 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 = From these data, the rate constant is M-1s-1.
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:AsO33- + 2 Ce4+ + H2OAsO43- + 2 Ce3+ + 2 H+ Experiment [AsO33-]o, M [Ce4+]o, M Initial Rate, M s-1 1 2.46×10-2 0.568 3.87×10-3 2 4.92×10-2 0.568 7.75×10-3 3 2.46×10-2 1.14 1.56×10-2 4 4.92×10-2 1.14 3.12×10-2 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , 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 = From these data, the rate constant is M-2s-1.