A. Reaction Rate Data: Mixture Vol.4.0M Vol Vol acetone 1.0M (mL) HCI (mL) 1 2 3 4 1 2 3 4 m = n= P= 10 20 10 Mixture 10 k= 10 10 10 Vol Total 0.0050M water solution volume (mL) loding (mL) (mL) rate= k(acetone)(H*)( iodine) P 의의의미 20 10 5 B. Determination of Reaction Orders with respect to Reagent Concentrations: Mixture [acetone] CH² [lodine) 0.80 0.0010 1.60 0.0010 0.80 0.0010 0.80 0.0005 C. Determination of Rate Constant (k): 1 2 20 50 10 50 10 25 50 0.20 0.20 0.40 0.20 3 Trial 1: Trial 2: Time of Time of reaction reaction (sec) (sec) (sec) 50 180.0 198.0 189.0 Ave. Time of reaction CC) 322.8 334.2 328.5 21°C 149.4 145.8 147.6 21°C. alºc 154.2 154.80 154.5 21°C 4 Temp. Reaction rate Average
A. Reaction Rate Data: Mixture Vol.4.0M Vol Vol acetone 1.0M (mL) HCI (mL) 1 2 3 4 1 2 3 4 m = n= P= 10 20 10 Mixture 10 k= 10 10 10 Vol Total 0.0050M water solution volume (mL) loding (mL) (mL) rate= k(acetone)(H*)( iodine) P 의의의미 20 10 5 B. Determination of Reaction Orders with respect to Reagent Concentrations: Mixture [acetone] CH² [lodine) 0.80 0.0010 1.60 0.0010 0.80 0.0010 0.80 0.0005 C. Determination of Rate Constant (k): 1 2 20 50 10 50 10 25 50 0.20 0.20 0.40 0.20 3 Trial 1: Trial 2: Time of Time of reaction reaction (sec) (sec) (sec) 50 180.0 198.0 189.0 Ave. Time of reaction CC) 322.8 334.2 328.5 21°C 149.4 145.8 147.6 21°C. alºc 154.2 154.80 154.5 21°C 4 Temp. Reaction rate Average
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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Please help me calculate the missing values!
![A. Reaction Rate Data:
Mixture
1
2
3
4
1
2
3
4
m=
n=
P=
Vol 4.0M Vol
acetone 1.0M
(mL) HCI
(mL)
10
20
10
Mixture
10
k=
rate= k(acetone)(H*)(i
(iodine) P
10
10
10
20 10
10 50
10 5 25 50
Total
Vol
Vol
0.0050M water solution
ieding (mL) volume
(mL)
(mL)
50
50
10
B. Determination of Reaction Orders with respect to Reagent Concentrations:
Mixture
[acetone]
[H*]
[iodine]
0.80
0.20
0.0010
1.60
0.20
0.0010
0.80 0.40
0.80
0.20
C. Determination of Rate Constant (k):
1
2
20
10
3
Trial 2:
Time of
Trial 1:
Time of
reaction reaction (sec)
(sec)
(sec)
322.8 334.2 328.5 21°C
149.4 145.8 147.6 21°C
180.0 198.0 189.0 21°C
154.2 154.80 154.5 21°C
Ave. Time
of reaction
0.0010
0.0005
4
Reaction rate
Temp.
(°C)
Average](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9a14a4fe-84d4-4d9d-934f-c00bddb83415%2F5a3b924a-5d71-418c-bc4b-1b99380684ec%2Fby6txxi_processed.png&w=3840&q=75)
Transcribed Image Text:A. Reaction Rate Data:
Mixture
1
2
3
4
1
2
3
4
m=
n=
P=
Vol 4.0M Vol
acetone 1.0M
(mL) HCI
(mL)
10
20
10
Mixture
10
k=
rate= k(acetone)(H*)(i
(iodine) P
10
10
10
20 10
10 50
10 5 25 50
Total
Vol
Vol
0.0050M water solution
ieding (mL) volume
(mL)
(mL)
50
50
10
B. Determination of Reaction Orders with respect to Reagent Concentrations:
Mixture
[acetone]
[H*]
[iodine]
0.80
0.20
0.0010
1.60
0.20
0.0010
0.80 0.40
0.80
0.20
C. Determination of Rate Constant (k):
1
2
20
10
3
Trial 2:
Time of
Trial 1:
Time of
reaction reaction (sec)
(sec)
(sec)
322.8 334.2 328.5 21°C
149.4 145.8 147.6 21°C
180.0 198.0 189.0 21°C
154.2 154.80 154.5 21°C
Ave. Time
of reaction
0.0010
0.0005
4
Reaction rate
Temp.
(°C)
Average
Expert Solution
Step 1
The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate equation of a chemical reaction. It is used to describe the dependence of the reaction rate on the concentration of the reactants.
The overall order of a reaction is the sum of the individual orders for each reactant.
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