A. Influence of Concentration on Reaction Rates Table 1: Trial 1 2 3 1. 2. Volume KIO3 (Flask #1) 20.0 mL 20.0 mL 30.0 mL (Note: Total volume is always 60.0 mL) A Volume Initial Concentration water (Flask #1) 30.0 mL Rate 2 Rate 3 20.0 mL 10.0 mL Volume NaHSO3 (Flask #2) Rate 1 Rose 2 (KIO₂ (2)]* 10.0 mL 20.0 mL 20.0 mL (right after mixing)/M [KIO3] 0, 03125 5¹ => Hauslovs 0.0556 0.058651 0.618 0.01 0.01 0.015 What is the order of this reaction in IO3- ? Show your calculations. (1103(1)] [001] [0.01) [NaHSO3] X 0.0083 0.0167 0.0167 1.855 What is the order of this reaction in HSO3- ? Show your calculations. t Reaction Time/s 1325 17.98 S 11.90 S Reaction Rate/s-1 7 0.0312551 0.05566-1 0.084 5-1 Lonctant for each of the three trials. Report the mean value of k and its ut fimures
A. Influence of Concentration on Reaction Rates Table 1: Trial 1 2 3 1. 2. Volume KIO3 (Flask #1) 20.0 mL 20.0 mL 30.0 mL (Note: Total volume is always 60.0 mL) A Volume Initial Concentration water (Flask #1) 30.0 mL Rate 2 Rate 3 20.0 mL 10.0 mL Volume NaHSO3 (Flask #2) Rate 1 Rose 2 (KIO₂ (2)]* 10.0 mL 20.0 mL 20.0 mL (right after mixing)/M [KIO3] 0, 03125 5¹ => Hauslovs 0.0556 0.058651 0.618 0.01 0.01 0.015 What is the order of this reaction in IO3- ? Show your calculations. (1103(1)] [001] [0.01) [NaHSO3] X 0.0083 0.0167 0.0167 1.855 What is the order of this reaction in HSO3- ? Show your calculations. t Reaction Time/s 1325 17.98 S 11.90 S Reaction Rate/s-1 7 0.0312551 0.05566-1 0.084 5-1 Lonctant for each of the three trials. Report the mean value of k and its ut fimures
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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. Influence of Concentration on Reaction Rates
Table 1:
Trial
1
2
3
1.
2.
Volume
KIO3
(Flask #1)
20.0 mL
20.0 mL
30.0 mL
(Note: Total volume is always 60.0 mL) A
Volume
Initial Concentration
water
(Flask #1)
Rate 2
Rate 3
30.0 mL
20.0 mL
10.0 mL
Volume
NaHSO3
(Flask #2)
10.0 mL
20.0 mL
20.0 mL
(right after mixing)/M
[KIO3]
0, 03125 5¹
=)
0.058651
Boliglove 032
0.618
0.01
0.01
0.015
What is the order of this reaction in IO3- ? Show your calculations.
Rate 1
(1105 (1)]
Rose 2 (KIO₂ (2)]*
:
[001]
[0.01)
[NaHSO3]
X
0.0083
0.0167
0.0167
1.855
What is the order of this reaction in HSO3- ? Show your calculations.
t
Reaction
Time/s
VER
1325
17.98 5
11.90 s
Reaction
Rate/s-1
7
0.031255-1
0.05566-1
0.084 5-1
constant for each of the three trials. Report the mean value of k and its
ut fimures](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7b47dd07-9dca-411e-981f-312dfe7288cb%2F0e435277-24a2-4320-87b9-990e2753645c%2Fqdyvjul_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A. Influence of Concentration on Reaction Rates
Table 1:
Trial
1
2
3
1.
2.
Volume
KIO3
(Flask #1)
20.0 mL
20.0 mL
30.0 mL
(Note: Total volume is always 60.0 mL) A
Volume
Initial Concentration
water
(Flask #1)
Rate 2
Rate 3
30.0 mL
20.0 mL
10.0 mL
Volume
NaHSO3
(Flask #2)
10.0 mL
20.0 mL
20.0 mL
(right after mixing)/M
[KIO3]
0, 03125 5¹
=)
0.058651
Boliglove 032
0.618
0.01
0.01
0.015
What is the order of this reaction in IO3- ? Show your calculations.
Rate 1
(1105 (1)]
Rose 2 (KIO₂ (2)]*
:
[001]
[0.01)
[NaHSO3]
X
0.0083
0.0167
0.0167
1.855
What is the order of this reaction in HSO3- ? Show your calculations.
t
Reaction
Time/s
VER
1325
17.98 5
11.90 s
Reaction
Rate/s-1
7
0.031255-1
0.05566-1
0.084 5-1
constant for each of the three trials. Report the mean value of k and its
ut fimures
Expert Solution
Step 1 Introduction
The order of a reaction is a measure of the rate at which a chemical reaction occurs with respect to the concentration of the reactants. It describes how the rate of the reaction changes when the concentration of one or more reactants is changed.
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