The following initial rate data are for the reaction of ICI with hydrogen: 21C1+ H₂ → I2+ 2HCl Experiment [IC]o, M [H₂lo, M Initial Rate, M s-1 0.397 0.202 0.0296 0.794 0.202 0.0593 0.397 0.404 0.119 0.794 0.404 0.237 1 2 3 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 n. Rate = k = M-2. 8-1

The following initial rate data are for the reaction of ICI with hydrogen: 21C1+ H₂ → I2+ 2HCl Experiment [IC]o, M [H₂lo, M Initial Rate, M s-1 0.397 0.202 0.0296 0.794 0.202 0.0593 0.397 0.404 0.119 0.794 0.404 0.237 1 2 3 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 n. Rate = k = M-2. 8-1

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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Given the following information about a reaction with a reactant A: Time (s) 0.0 6.0 12.0 18.0 [A](M) 1.22 0.61 0.31 0.15 What is the initial rate of the reaction (rate from 0.0 s - 6.0 s)?
The following initial rate data are for the reduction of nitric oxide with hydrogen:2 NO + 2 H2N2 + 2 H2O Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.160 0.420 1.57×10-2 2 0.320 0.420 6.28×10-2 3 0.160 0.840 3.14×10-2 4 0.320 0.840 0.126 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
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
6) The decomposition of reactant R was studied, and the data given below was obtained at 100.0 °C: R> products time (min) concentration (M) 0.120 35.6 5.83 17.8 25.6 0.0910 0.060 0.046 0.030 a) What is the half-life of the reaction in minutes? Explain. b) Various plots of the concentration of the reactant versus time are given below. What is the order of the reaction? Explain. ILD is 20 time (min) time (min) 05 -35 time (min) c) What is the value of the rate constant at 100.0 °C? d) Would you expect the half-life of the reaction to be longer, shorter, or the same at 60.0 °C? Explain. e) The activation energy in the forward direction is 95.0 kl/mol, and the enthalpy change for the forward reaction is 30.0 kl/mol. Sketch the reaction coordinate diagram for this reaction. ERER AR
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The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2- →I2 + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, M s-1 1 0.339 7.80x10-2 |3.63х10-3 0.678 7.80x10-2 7.26x10-3 3 0.339 0.156 1.45x10-2 14 0.678 0.156 2.90x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[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-2s-1.
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂ + 2 H₂O Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1 0.0358 1.45 x 10-6 0.0715 0.0358 0.0715 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 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. k = 2.89 x 10-6 2.88 x 10-6 5.76 x 10-6 M-1.s-1
The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO + 03 NO₂ + O₂ Experiment [NO]o, M [03]o, M Initial Rate, M-s1 0.192 0.0497 0.928 0.192 0.0994 1.86 0.384 0.0497 1.86 0.384 0.0994 3.71 1 2 3 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
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.113 3.10×10-2 1.81×10-4 2 0.226 3.10×10-2 3.63×10-4 3 0.113 6.20×10-2 7.25×10-4 4 0.226 6.20×10-2 1.45×10-3 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 = k_____ From these data, the rate constant is ______M-2s-1.
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 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.
7 11 The initial rate of the reaction has been measured at the reactant concentrations show: Trial [BrO3] [H*] (mol/L) (mol/L) 0.10 0.10 0.20 0.10 0.10 0.20 0.10 0.10 1 23 3. 4 The rate law expression will be: [Br] (mol/L) 0.10 0.10 0.10 0.20 Initial rate (mol/L.s) 8.0 16 16 32
The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO+O3 → NO₂ + O2 Experiment [NO]o, M [03]0, M Initial Rate, M s . 0.147 0.0234 0.344 0.147 0.0468 0.688 0.294 0.0234 0.688 0.294 0.0468 1.38 1 2 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 = k = 1 M-¹ S 1 1