napters 9 and 11)[References]The following experimental data were obtained for the reaction of NH4* and NO2- in acidicsolution.NH, “ (aq) + NO, -(aq) → N2 (g) + 2 H20(t)[NH, +] (mol L-1) NO, ] (molL-1) Rate =A[N2]/At (mol L-10.00170.1305.53 x 10-80.00172.76 x 10-80.0650.00905.86 x 10-70.2600.00460.2602.98 x 10-7Determine the rate law for this reaction.(Use k for the rate constant.)Rate =Calculate the rate constant.Rate constant =Submit AnswerTry Another Version10 item attempts remaining

pters 9 and 11) References) The following experimental data were obtained for the reaction of NH,* and NO,- in acidic solution. NH, "(aq) + NO, (aq) → N2 (g) + 2 H2O(4) [NH, *] (mol L) NO, ] (mol L-) Rate = A[N2]/At (mol L-s 0.0017 0.130 5.53 x 10-8 0.0017 0.065 2.76 x 10-8 0.0090 0.260 5.86 x 10-7 0.0046 0.260 2.98 x 10-7 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =| Submit Answer Try Another Version 10 item attempts remaining

pters 9 and 11) References) The following experimental data were obtained for the reaction of NH,* and NO,- in acidic solution. NH, "(aq) + NO, (aq) → N2 (g) + 2 H2O(4) [NH, *] (mol L) NO, ] (mol L-) Rate = A[N2]/At (mol L-s 0.0017 0.130 5.53 x 10-8 0.0017 0.065 2.76 x 10-8 0.0090 0.260 5.86 x 10-7 0.0046 0.260 2.98 x 10-7 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =| Submit Answer Try Another Version 10 item attempts remaining

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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chemical kinetics
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Date: Rate-Law Hand-In D 1. The reaction below takes place in aqueous solution: 2 CIO, + 2 OH → CIO, + CIO, + H,O The following observation were made: EXP. # Initial [CIO;] Initial [OH:] Initial rate (mol/L-s) 1 0.1 0.2 0.2 0.2 0.1 0.45 1.84 0.92 0.2 a. Write the rate law for this reaction. b. What is the order of the reaction with respect to each of the reactants? C. What is the overall order of the reaction? -23
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amples: Unimeleculo gras a Teact Eimaan e - Rea 1) A chemical reaction proceeds with the proposed reaction mechanism below; Step Kinetics Assignment SCH4U0 E (kJ/mol) 75AH +175 25-AH +50 N2e) + Oze) → N,O« +O«). 1 +25 -150+0H N2O +Oz«) → NOe) +NO) NOw +O«) → N0ze) a) Draw the potential energy diagram for this reaction below. 300 250 P. E. 200 (k J/ 150 mo 1) 100 +0218) 50 b) What is the overall reaction? N2 9) + 2 Ozcg -> c) Which step is the rate determining step? Explain why. Step 2 because it has the highest activation energy. d) What would be the rate law for this reaction? K= [ e) Explain what would happen to the rate if the concentration of Ne doubled. f) Use a dotted line to show what would happen if a catalyst was added to the reaction. g) Identify the spot on the graph that represents the transition state for reaction 2. h) Identify the intermediates present in this reaction. (Intermediates are produced and consumed in the reaction mechanisms)
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For the reaction 2NOCI 2NO + Cl, the rate constant k equals 0.020 L mol-1 s1 at a certain temperature. Determine how many minutes it would take for the NOCI concentration to drop from 0.091 M to 0.063 M. It would take i minutes. eTextbook and Media Hint Last saved 16 minutes ago. Attempts: 3 of 15 used Submit AnswE Save for Later Saved work will be auto-submitted on the due date. Auto- submission can take up to 10 minutes. P A O S