The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: As033 + 2 Ce4+ + H20 As0,3 + 2 Ce3+ + 2 H+ Experiment [As033lo, M [Ce*Jo, M Initial Rate, Ms 1 4.91x10 2 0.461 5.74x10 3 2 9.82x10 2 0.461 1.15×10 2 4.91x10 2 0.922 2.30x10 2 4 9.82x10 2 0.922 4.59x10 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 M25 1

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: As033 + 2 Ce4+ + H20 As0,3 + 2 Ce3+ + 2 H+ Experiment [As033lo, M [Ce*Jo, M Initial Rate, Ms 1 4.91x10 2 0.461 5.74x10 3 2 9.82x10 2 0.461 1.15×10 2 4.91x10 2 0.922 2.30x10 2 4 9.82x10 2 0.922 4.59x10 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 M25 1

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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v Question Completion Status: Question 21 The reaction CO + Cl2 - COCI2 was studied by the initial rate method and the following data were obtained: Initial Rate [CO), (M) [Cl2], (M) (mol/Lxs) 1.00 x 10-2 1.00 × 10-2 6.60 x 103 3.00 x 10-2 1.00 × 10-2 1.98 x 104 1.00 x 10-2 4.00 × 10-2 1.06 x 105 The rate law is: rate = k[COj?{Cl2] O rate = k[CO][Cl2]1/2 O rate = k[Cl2] O rate = k[CO][Cl2)2 O rate = k[CO][Cl2] S15 A Click Submit to complete this assessment. MacBook Air Breathe easy.
For Questions 4 and 5, consider the following kinetic data for the decomposition of N204 into NO2. Specific-rate constant, k (s-1) Temperature (°C) -5 2.5 x 103 25 3.5 x 104 5.) What is the numerical value of the activation energy (in kJ/mol) for this reaction?
4-chem The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO,- + 2 Ce*+ + H2O→ASO,³- +2 Ce³+ + 2 H† Experiment [AsO,lo, M [Ce**]o, M -1 Initial Rate, M s 7.21x10-3 1.44x102 7.21×10-3 1.44x102 1 0.514 9.98×10-4 2 0.514 1.99x103 1.03 4.01×10-3 14 1.03 8.01×10-3 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
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Aso,3 + 2 Ce** + H20-Aso,3 + 2 Ce3* + 2 H* Initial Rate, M Experiment [Aso,3-], M [Ce**1, M Is 8.53x104 1.71x10-3 3.41x103 6.83x103 1 3.61x10-2 0.204 7.22x10-2 3.61x102 7.22x10-2 2 0.204 3 0.408 14 0.408 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. Rate = From these data, the rate constant is M2s1.
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 activation energy? rate = r = k [I-]^1 [S2O82-]^1 Mixtures: Temperatures (celsius): Initial Rates: 1 21.9 6.45 * 10-4 2 38.9 3.54 * 10-4 3 2.4 4.35 * 10-4
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: As033- + 2 Ce4+ + H20→AS043- + 2 Ce3+ + 2 H+ Experiment [As033-]o, M [Ce4+]o, M Initial Rate, M s1 2.86x10-2 4.52x10-3 1 0.545 2 5.72x10-2 0.545 9.04x10-3 2.86x10 2 1.81x10-2 3 1.09 5.72x10-2 3.62x10-2 4 1.09 Complete the rate law for this reaction in the box below. Use the form k[A]™[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-25-1.
If the y-axis of the graph changes to “volume of hydrogen / cm3 ”, sketch this rate curve. What will be the effect on the reaction rate if the concentration of HCl changes from 0.1 M to 0.2 M? Explain
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Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
Values if needed for this question. The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion: 2 HgCl2 + 2 CI + Hg,Cl2 + 2 CO2 Experiment [HgCl2]o, M [C,0,?], M Initial Rate, M sl 1 0.415 0.180 1.23x104 0.830 0.180 2.45x104 4.91×10-4 9.81×104 3 0.415 0.360 4 0.830 0.360 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 power not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1 Submit Answer Try Another Version 2 item attempts remaining