You perform a "Clock" reaction experiment using a similar Initial Rate Method and obtain the following data: Run# Reactant A Reactant B Time to Blue 1 0.100 M 0.100 M 80.0 seconds 2 0.300 M 0.100 M 80.0 seconds 3 0.100 M 0.200 M 20.0 seconds The order with respect to A is [ Select ] The order with respect to B is v [ Select ] Second Order Zero Order First Order

You perform a "Clock" reaction experiment using a similar Initial Rate Method and obtain the following data: Run# Reactant A Reactant B Time to Blue 1 0.100 M 0.100 M 80.0 seconds 2 0.300 M 0.100 M 80.0 seconds 3 0.100 M 0.200 M 20.0 seconds The order with respect to A is [ Select ] The order with respect to B is v [ Select ] Second Order Zero Order First Order

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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A certai.. cuction is second order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [#.] H initial rate of reaction х10 2.01 M 2.18 M 99.0 M/s 3.07 M 2.18 M M/s ||M/s O Mls 0.483 M 9.07 M
The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C: 2 NO + O2- →2 NO2 Experiment NO],, M [02lo, M Initial Rate, M s 5.86x103 1.17x10-2 4.59x10-3 1.29x10-3 5.15x10-3 2.58x10-3 4.59x10-3 9.18x10-3 9.18×10-3 3 5.86x10-3 1.17x10-2 1.03x10-2 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 %D
The following initial rate data were found for the reaction 2MnO4 +5H₂C2O4 + 6H+ → 2 Mn²+ [-] (M) {H+] (M) 1.00×10-3 1.0 1.00×10-3 1.0 2.00×10-3 1.0 2.00×10-3 2.0 Experiment 1 [MnO4-] (M) 1.00×10-3 2.00×10-3 2.00×10-3 2.00×10-3 The rate law for this reaction is 2 (ر) Rate = k[MnO4]²[H₂C₂O4][H+] Rate = k[MnO4]²[H₂C₂O4]5[H+]6 Rate = k[MnO4]²[H₂C₂O4] Rate = k[MnO4][H₂C₂O4][H+] Rate = k[MnO4]²[H₂C₂O4]² + 10 C Rate (M/s) 2.0×10-4 8.0×10-4 1.6x10-3 1.6×10-3
A certain reaction is second order in N₂ and second order in H₂. Use this information to complete the table below. Be sure each of your answer entries ha correct number of significant digits. 1.65 M 1.65 M 0.187 M Explanation 0.450 M 1.60 M 3.96 M initial rate of reaction Check 6.00 x 10 Mis 16 Mis Mis O x10 X tv w MacBook Air 3/5 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center
Combination # [IO3-]0 [H+]0 [I-]0 average dt(sec) Initial rate, M s-1 kR (including units) 1 0.010 0.00002 0.10 18.1 0.00055 2 0.020 0.00002 0.10 9.1 0.0022 3 0.010 0.00002 0.20 5.1 0.0020 4 0.010 0.00002 0.10 5.1 0.0020 1. Determine the orders x,y and z 2. Calculatethe rate constant, kR and average kR for combimnations 1-4 3. Write the experimenally determined rate law Rate =kR[IO3-]x [I-]y [H+]z
Consider the reaction: 2 A + B " C + 3 DThe following data are obtained at 25°C: Experiment # [A]0 [B]0Initial rates(mol L-1 s-1)10.10 0.10 1.25 x 10-720.10 0.20 5.00 x 10-730.20 0.20 1.00 x 10-6a. Determine the order of the reaction with respect to each reactant and overall. b. Determine k, the rate constant. c. Give the rate law for this reaction. d. Suggest a plausible mechanism for this reaction that is consistent with the rate law.
[A] vs Time In[A] vs Time 1/[A] vs Time Least Squares Plot Time, s The reaction A - C was performed and the concentration vs. time data below collected. time, s 2 4 5 7 8. [A], mol/L 0.7041 0.4665 0.3091 0.2048 0.1357 0.08988 0.05955 0.03946 0.02614 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]* rate constant (without units) = || reaction order In[A]
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5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
For the given data, what is the correct unit for the rate constant, k? Run [B] [C] Initial Rate (M/sec) 1 1.5 2.0 0.20 2 1.5 4.0 0.40 3 3.0 2.0 0.80
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please help part B