3. The decomposition of N2O5 in the gas phase was studied at constant temperature,2N2O5 (g) → 4NO2 (g) + O2(g)The following results were collected:findnature)N2O5]0.1000Ln[N2O5]-2.302.652.99-3.69-4.38-5.08a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time andTime (s)10g.(LN)0.07070.0500500.02501000.01252000.00625300400Ln[N2O5] versus time. Determine the value of k. Which graph didyou use?graph*b. On your graph of [N2O5] versus time, highlight the times it takes for each halving ofthe reactant concentration. What is the half-life? Using this half-life calculate k.design experiments to find the activation energy, KInetics Problems Laboratory1. Using the following chemical equation and data:A=Second order reactantB-first order reactantSimilarto3A + B+ 2C →D+2EExperimentnotesExамpleInitial [A]1.0 x 1021.0 x 1022.0 x 1022.0 x 102Initial [B]4.0 x 1038.0 x 1038.0 x 10-38.0 x 10-3Initial [C]2.0 x 1022.0 x 1022.0 x 10,21.0 x 1021Initial Rate25 mM/s310 mM/s *40 mM/s *40 mM/s4Determine the rate equation.b. Calculate the specific rate constant (k).Determine the initial rate of reaction if the initial concentrations of A, B, C are3 x 102 M, 5 x 10-3 M, 5 x 103M, respectively, for the reaction.a.с.a.) Rate= [A]²CB]'b.) K= rateCAJ C6]' = 5 m/s(10x (0-2) 2 (4.0x10-3)'=2M!5-1%3DC.)2. The reaction between bromate ions and bromide ions in acidic aqueous solution is givenby the following equation:BrO3 (aq) + 5Br (aq) +6H* (aq) → 3B12 (1) + 3H2O (1)

Since you have asked multiple questions, we will solve the first question for you. If you want any…

3. The decomposition of N2O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO2 (g) + O2(g) The following results were collected: find nature log. (LN) N2O5] 0.1000 Ln[N2O5] -2.30 -2.65 -2.99 -3.69 -4.38 Time (s) 0.0707 0.0500 50 0.0250 100 0.0125 200 0.00625 300 400 .08 a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and Ln[N2O5] versus time. Determine the value of k. Which graph did graph *b. On your graph of [N2O5] versus time, highlight the times it takes for each halving of you use? the reactant concentration. What is the half-life? Using this half-life calculate k.

3. The decomposition of N2O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO2 (g) + O2(g) The following results were collected: find nature log. (LN) N2O5] 0.1000 Ln[N2O5] -2.30 -2.65 -2.99 -3.69 -4.38 Time (s) 0.0707 0.0500 50 0.0250 100 0.0125 200 0.00625 300 400 .08 a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and Ln[N2O5] versus time. Determine the value of k. Which graph did graph *b. On your graph of [N2O5] versus time, highlight the times it takes for each halving of you use? the reactant concentration. What is the half-life? Using this half-life calculate k.

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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Question

3. The decomposition of N2O5 in the gas phase was studied at constant temperature,
2N2O5 (g) → 4NO2 (g) + O2(g)
The following results were collected:
find
nature)
N2O5]
0.1000
Ln[N2O5]
-2.30
2.65
2.99
-3.69
-4.38
-5.08
a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and
Time (s)
10g.
(LN)
0.0707
0.0500
50
0.0250
100
0.0125
200
0.00625
300
400
Ln[N2O5] versus time. Determine the value of k. Which graph did
you use?
graph
*b. On your graph of [N2O5] versus time, highlight the times it takes for each halving of
the reactant concentration. What is the half-life? Using this half-life calculate k.
design experiments to find the activation energy,

KInetics Problems Laboratory
1. Using the following chemical equation and data:
A=Second order reactant
B-first order reactant
Similar
to
3A + B+ 2C →D+2E
Experiment
notes
Exамple
Initial [A]
1.0 x 102
1.0 x 102
2.0 x 102
2.0 x 102
Initial [B]
4.0 x 103
8.0 x 103
8.0 x 10-3
8.0 x 10-3
Initial [C]
2.0 x 102
2.0 x 102
2.0 x 10,2
1.0 x 102
1
Initial Rate
2
5 mM/s
3
10 mM/s *
40 mM/s *
40 mM/s
4
Determine the rate equation.
b. Calculate the specific rate constant (k).
Determine the initial rate of reaction if the initial concentrations of A, B, C are
3 x 102 M, 5 x 10-3 M, 5 x 103M, respectively, for the reaction.
a.
с.
a.) Rate= [A]²CB]'
b.) K= rate
CAJ C6]' = 5 m/s
(10x (0-2) 2 (4.0x10-3)'=2M!5-1
%3D
C.)
2. The reaction between bromate ions and bromide ions in acidic aqueous solution is given
by the following equation:
BrO3 (aq) + 5Br (aq) +6H* (aq) → 3B12 (1) + 3H2O (1)

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a. Graph of [N2O5] versus time

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Determining the value of k

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3.
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