03_ReactionRates_PostLab_Spring 24
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Reaction Rates
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CHM 116 POST-LAB
Reaction Rates: Determining Order of Reactants and Rate Law
1.
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include the 24 -Well plate) in your PPE picture
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2.
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Materials
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Determining Rate Law
This reaction rate data is analyzed and used to determine the rate law for the reaction between HCl and Na
2
S
2
O
3
.
2HCl(aq) + Na
2
S
2
O
3
(aq) → S(s) + SO
2
(aq) + H
2
O(l) + 2NaCl(aq)
The general form for the rate law for the above reaction between HCl and Na
2
S
2
O
3
is written as:
Rate = k[
HCl
]
x
[
Na
2
S
2
O
3
]
y
When the concentration of one chemical is changed, the other chemical’s concentration
is held constant. When testing for the order of [HCl], [Na
2
S
2
O
3
]
is held constant. When testing for [Na
2
S
2
O
3
], [HCl] is held constant. This means that any change in reaction rate between experiments can be attributed to the change in just one of the reactants (the other is held constant).
In doing so, the variables m and n can be separately computed via a ratio.
Part 1: Determining Order for HCL
3.
Data Table 1: Varying the concentration of HCl while keeping the concentration of Na
2
S
2
O
3
constant.
Table 1: Varying the concentration of HCl
Number of drops
Concentrations (M)
Reaction Time(sec)
Reaction Rate
Well #
HCl
Water
Na
2
S
2
O
3
HCl
initial
Na
2
S
2
O
3
initial
HCl
final
Na
2
S
2
O
3
final
Trial
1
Trial
2
Average
Sec
-1
C1, D1
12
0
8
1M
0.3 M
0.6 M
0.12 M
23.9
23.4
23.65
0.42
C2, D2
6
6
8
0.5 M
0.3 M
0.3 M
0.21 M
31.4
28.6
30.0
.033
C3, D3
4
8
8
0.33 M
0.3M
34.6 M
32.6 M
34.6
32.6
33.6
.029
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4.
Show your work for the following calculations:
Determine the concentration (in molarity) of HCl and the concentration (in molarity) of Na
2
S
2
O
3
for each experiment in Part 1. These are just dilution calculations.
5.
Show your work for the following calculations:
Determine the initial reaction rate for each experiment in Part 1.
Calculated [HCl] for
:
Wells C1 and D1:
Wells C2 and D2:
Wells C3 and D3:
Calculated [
Na
2
S
2
O
3
] for all wells (C1, D1, C2, D2, C3, D3)
:
Average Reaction Times
:
Wells C1 and D1:
Wells C2 and D2:
Wells C3 and D3:
Initial Reaction Rates:
Wells C1 and D1:
Wells C2 and D2:
Wells C3 and D3:
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6.
Using the data from Table 1
, find the reaction order of HCl. This value is the “
x
” in the rate law for the reaction:
Rate = k[
HCl
]
x
[
Na
2
S
2
O
3
]
y
Use the initial rate
of two experiments in which the concentration of HCl varied (from Table 1), but the concentration of Na
2
S
2
O
3
stayed the same. (use the Introduction document for reference). Show your work.
Part 2: Determining Order for Na
2
S
2
O
3
7.
Data Table 2: Varying the concentration of Na
2
S
2
O
3 while keeping the concentration of
HCl constant.
Table 2: Varying the Concentration of Na
2
S
2
O
3
Number of drops
Concentrations (M)
Reaction Time(sec)
Initial
Reaction
Rate
Well #
HCl
Water
Na
2
S
2
O
3
HCl
initial
Na
2
S
2
O
3
initial
HCl
final
Na
2
S
2
O
3
final
Trial 1
Trial 2
Average
Sec
-1
C4, D4
8
0
12
1 M
0.3 M
0.6 M
0.18 M
18.1
18.5
18.3
.054
C5, D5
8
6
6
1 M
0.15 M
0.07
M
0.09 M
34.0
40.0
37.0
.027
C6, D6
8
8
4
1 M
0.1 M
0.8 M
0.06 M
59.0
65.1
62.05
.016
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8.
Show your work for the following calculations:
Determine the concentration (in molarity) of HCl and the concentration (in molarity) of Na
2
S
2
O
3
for each experiment in Part 2. These are just dilution calculations.
9.
Using the whole number values calculated in Questions 6 and 10, write down the rate law expression
with the respective reaction orders for HCl and Na
2
S
2
O
3
. Calculated [
Na
2
S
2
O
3
] for
:
Wells C4 and D4:
Wells C5 and D5:
Wells C6 and D6:
Calculated [
HCl
] for all wells (C4, D4, C5, D5, C6, D6)
:
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Rate= k[Na2S2O3]1[HCL]0
116 Online Lab Notebook Entry ( 5 Points)
Purpose/Goal of Experiment:
Planned Observations:
Experiment Title:
__________________________________________________
Date of Experiment:
__________________________________________________
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__________________________________________________
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Qualitative/ Quantitative Observations:
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Data/Calculations:
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Conclusion:
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Hint
Attempts: 1 of 3 used
Your Answer
Correct Answer (Used)
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Date:
Section:
Data Report Sheet: The Reaction of Methyl Violet with NaOH: A Kinetic
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Related Questions
- 0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HIarrow_forwardWhen fitting data to a best fit line, a correlation coefficient (R2) is determined and used to evaluate the quality of fit. The best fit of the data will have an R² value closest or equal to zero (0). closest or equal to one (1). equal to the rate of the reaction occurring. equal to the rate constant of the reaction occurring.arrow_forwardA + 2B -> C (rate constant = k1, rA = -k1[A][B]2) C -> A + 2B (rate constant = k-1, rA = k-1[C]) C + 2A -> 2D (rate constant = k2, rA = -k2[C][A]2) reaction rate constant and the rate for A of each elementary reaction are shown in the parentheses after each reaction. Calculate the overall reaction rate for A in terms of [A], [B], k1, k-1, and k2 assuming c is psuedo-state-concentration overall chemical rxn is 3A+2B->2Darrow_forward
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