The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °CNO + O3NO, + 02Experiment[NO], M[031.. MInitial Rate, Ms10.1324.69x10-20.5870.1329.38x101.170.2654.69x10-1.1840.2659.38x1022.36Complete 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 thezero power do not appear. Don't enter 1 for m or nRate =From these data, the rate constant isSubmit AnswerRetry Entire Group9 more group attempts remainingPreviousNeEmail Instructor

The rate of a reaction can be defined as the rate of decrease in concentration of reactants or the…

The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C NO + O3 →NO2 + 02 Experiment [NO], M [03]., M Initial Rate, Ms 1 0.132 4.69x102 0.587 12 0.132 9.38×10- 1.17 0.265 4.69x102 1.18 4 0.265 9.38×10- 2.36 3.

The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C NO + O3 →NO2 + 02 Experiment [NO], M [03]., M Initial Rate, Ms 1 0.132 4.69x102 0.587 12 0.132 9.38×10- 1.17 0.265 4.69x102 1.18 4 0.265 9.38×10- 2.36 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...

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For this reaction occurring at 20 °C, the following data was obtained. C6H12O + Br2 → C6H11OBr + HBr What is the rate law of the reaction? Run C6H12O (M) Br2 (M) Initial Rate, M/min 1 0.20 0.15 2.55 x 10-4 2 0.40 0.15 2.52 x 10-4 3 0.40 0.30 5.09 x 10-4
The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide: NO, + CO NO + CO, Experiment 1 NO:l,. M 1.28 [CO], M 0.457 0.914 Initial Rate, Ms- 1.06 1.06 lo 2 1.28 2.55 2.55 13 0.457 4.23 4 0.914 4.23 Complete the rate law for this reaction in the box below. Use the form k[A]mB]" , where 'l' 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 gas phase reaction of hydrogen with iodine: H₂+I₂ → 2 HI Experiment [H₂0, M120, M Initial Rate, M.s¹ 0.0212 0.0180 7.17 x 10-22 0.0212 0.0360 1.43 x 10-21 0.0424 0.0180 1.43 x 10-21 0.0424 0.0360 2.87 x 10-21 1 2 4 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 71. Rate = k= M-1
4. The following data were obtained for the follwing chemical reaction: 2A+38->2C+D Trial # Initial (A) Initial [B] Initial Rate of Formation (mmol/L) (mmol/L) of D (mmol/L."s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (T: 2) (b) Find the rate constant, k, with units. (T: 2)
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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
Time (h) IN,0,1 (mel/1) Time (h) DN0) (mel/L) 0.00 0.849 3.00 0.352 0,50 0.733 4.00 0.262 1.00 0.633 5.00 0.196 2.00 0.472 3. Using data given in the table for the reaction N,O, 2 NO, + 0, calculate the average rate over the interval 0 to 5.0h. Compare your result with the average rates over the intervals 1.0 to 4.0 h and 2.0 to 3.0 h, all of which have the same midpoint (2.5 h from the start).
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Kinetic data were obtained on the aqueous reaction of hydrogen peroxide with iodide ion and H+. H2O2(aq) + 3 l-(aq) + 2 H+(aq) → 13-(aq) + 2 H2O(1) Exp. 1 [H₂0₂], M 0.010 [I], M 0.010 [H+], M 0.00050 Initial Rate, M/s 1.15 x 10-6 2 0.020 0.010 0.00050 4.60 x 10-6 3 0.010 0.020 0.00050 1.15 x 10-6 4 0.010 0.010 0.00100 2.30 x 10-6 Determine the rate law for the reaction: none of the answers are correct R = 2.3 M-2 S-1 [H2O2]2 [H+] R = 1.15 x 10-2 M-1 S-1 [H2O2]2 R = 0.0115 M-1 S-1 [H2O2] [-]
Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 0.40 1.2 x 10-4 0.40 6.2 x 10-5 Initial rate (M/sec) 3.1 x 10-5 (a) Find the order of the reaction with respect to HgCl2₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.
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