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
How do you write the overall rate law with the k value specific to this reaction?
![2.
173
Table 12.2 Solutions for Kinetic Runs
Run
Flask A
Flask B
250 mL beaker
1.
20.00 mL 0.200 M KI
10.00 mL 0.00500 M Na2S2O3
5 drops starch
20.00 mL 0.100 M K2S;Os
10.00 mL 0.100 M K2S2OS
10.00 mL 0.100 M Na2SO4
10.00 mL 0.00500 M NazS2O3
5 drops starch
20.00 mL 0.200 M KI
15.00 mL 0.100 M K2S2O8
5.00 mL 0.100 M NazSO4
10.00 mL 0.00500 M Na2S2O3
5 drops starch
20.00 mL 0.200 M KI
3.
10.00 mL 0.200 M KI
4.
10.00 mL 0.200 KCI
10.00 mL 0.00500 M Na2S2O3
5 drops starch
20.00 mL 0.100 M K2S2O8
15.00 mL 0.200 M KI
5.00 mL 0.200 M KCI
10.00 mL 0.00500 M NazS2O3
5 drops starch
20.00 mL 0.100 M K2S2O8
For each of the above, measure the KI and the K,S,Os precisely from the burets. The
KCI and NazSO4 solutions are added only to keep the total ionic concentration in each
mixture the same. This is necessary to avoid secondary effects.
1. Calculate the initial concentrations of I, S,O2, and S2O, in each run using the data
in Table 12.2 and the dilution formula M,V1 = M2V2, is as follows:
(0.200 M)(20.00 mL)
0.0800 M
(50.00 mL)
(0.100 M)(20.00 mL)
30.0400 M
(50.00 mL)
(0.00500 M)(10.00 mL)
30.00100 M
%3D
(50.00mL)
2. Calculate A[l2]. From the indicator reaction equation, the concentration of S2O3 is
twice as great as the concentration of I2 produced in the time At. Therefore, the
concentration of I, produced in time At will be one-half the concentration of S2O3
initially present in the reaction solution.
2-
[o's]
[S,O,] = 1.00 x 103 M; therefore A[l2] = 5.00 x 10 M
%3D
3. Normalize and then fill four burets: one with 0.200M KI, one with 0.200 M KCI, one
with 0.100 M K2S2O§ and the remaining one with 0.100 M Na2SO4.
171
s dependent on temp
[S;O, Jo
Rate (A[I2]/At)
K.
Run
LO°s]
Units:
5.00 x 10-4
니1,0s
100m
2
0.0800 m
3.
0.0800 m
0.0400 m
82.0s
4.
5.
10.200m)(20.0mL) 0.100m)(20.00mL) Co.0050om)(0.00 mil l Ali,]: [5,0,],
50.00mL
2. Determine the order with respect to [S2Os ].
1. Determine the order with respěct to TI ].
3. Determine the overall order of the reaction.
4. Calculate the average k (with units). AllS Ks
5. Write the overall rate law expression with the k value specific to this reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb234898a-ca00-4740-ae3d-79576f672843%2Fed9299a8-4a8f-4144-a0b6-a0ca81084ec4%2Fsyyjw29.jpeg&w=3840&q=75)
Transcribed Image Text:2.
173
Table 12.2 Solutions for Kinetic Runs
Run
Flask A
Flask B
250 mL beaker
1.
20.00 mL 0.200 M KI
10.00 mL 0.00500 M Na2S2O3
5 drops starch
20.00 mL 0.100 M K2S;Os
10.00 mL 0.100 M K2S2OS
10.00 mL 0.100 M Na2SO4
10.00 mL 0.00500 M NazS2O3
5 drops starch
20.00 mL 0.200 M KI
15.00 mL 0.100 M K2S2O8
5.00 mL 0.100 M NazSO4
10.00 mL 0.00500 M Na2S2O3
5 drops starch
20.00 mL 0.200 M KI
3.
10.00 mL 0.200 M KI
4.
10.00 mL 0.200 KCI
10.00 mL 0.00500 M Na2S2O3
5 drops starch
20.00 mL 0.100 M K2S2O8
15.00 mL 0.200 M KI
5.00 mL 0.200 M KCI
10.00 mL 0.00500 M NazS2O3
5 drops starch
20.00 mL 0.100 M K2S2O8
For each of the above, measure the KI and the K,S,Os precisely from the burets. The
KCI and NazSO4 solutions are added only to keep the total ionic concentration in each
mixture the same. This is necessary to avoid secondary effects.
1. Calculate the initial concentrations of I, S,O2, and S2O, in each run using the data
in Table 12.2 and the dilution formula M,V1 = M2V2, is as follows:
(0.200 M)(20.00 mL)
0.0800 M
(50.00 mL)
(0.100 M)(20.00 mL)
30.0400 M
(50.00 mL)
(0.00500 M)(10.00 mL)
30.00100 M
%3D
(50.00mL)
2. Calculate A[l2]. From the indicator reaction equation, the concentration of S2O3 is
twice as great as the concentration of I2 produced in the time At. Therefore, the
concentration of I, produced in time At will be one-half the concentration of S2O3
initially present in the reaction solution.
2-
[o's]
[S,O,] = 1.00 x 103 M; therefore A[l2] = 5.00 x 10 M
%3D
3. Normalize and then fill four burets: one with 0.200M KI, one with 0.200 M KCI, one
with 0.100 M K2S2O§ and the remaining one with 0.100 M Na2SO4.
171
s dependent on temp
[S;O, Jo
Rate (A[I2]/At)
K.
Run
LO°s]
Units:
5.00 x 10-4
니1,0s
100m
2
0.0800 m
3.
0.0800 m
0.0400 m
82.0s
4.
5.
10.200m)(20.0mL) 0.100m)(20.00mL) Co.0050om)(0.00 mil l Ali,]: [5,0,],
50.00mL
2. Determine the order with respect to [S2Os ].
1. Determine the order with respěct to TI ].
3. Determine the overall order of the reaction.
4. Calculate the average k (with units). AllS Ks
5. Write the overall rate law expression with the k value specific to this reaction.
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