Run-1 Run-2 Run-3 Run-4 Average time(s) [H₂O2] (M) [I-](M) 210.6 74.3 314 82 Quantity [Na₂S₂O3] stock [KI] stock [H₂O₂] stock k' 0.04 0.04 0.0125 0.025 Value 0.005M 0.2M 0.1M INITIAL CONCENTRATION 0.0386 0.04 0.08 0.1 0.1 Run 1 Run 2 Run 3 Run 4 Na₂S₂O3 0.005M 1 drop 1 drop 1 drop 1 drop [S₂03²-] (M) 0.001 0.001 0.00125 0.00125 KI 0.1M 2 drops KI 0.2M 2 drops 2 drops 2 drops H₂O₂ 0.05M 1 drop Assuming that the colour change occurred at the moment the S₂03² was completely consumed, determine the average rate of disappearance of S₂O3²- during this reaction (for Run #1): From the rate of disappearance of S₂O3², determine the average rate of reaction for Run #1: H₂O₂ 0.1M 2 drops 2 drops 1 drop
Run-1 Run-2 Run-3 Run-4 Average time(s) [H₂O2] (M) [I-](M) 210.6 74.3 314 82 Quantity [Na₂S₂O3] stock [KI] stock [H₂O₂] stock k' 0.04 0.04 0.0125 0.025 Value 0.005M 0.2M 0.1M INITIAL CONCENTRATION 0.0386 0.04 0.08 0.1 0.1 Run 1 Run 2 Run 3 Run 4 Na₂S₂O3 0.005M 1 drop 1 drop 1 drop 1 drop [S₂03²-] (M) 0.001 0.001 0.00125 0.00125 KI 0.1M 2 drops KI 0.2M 2 drops 2 drops 2 drops H₂O₂ 0.05M 1 drop Assuming that the colour change occurred at the moment the S₂03² was completely consumed, determine the average rate of disappearance of S₂O3²- during this reaction (for Run #1): From the rate of disappearance of S₂O3², determine the average rate of reaction for Run #1: H₂O₂ 0.1M 2 drops 2 drops 1 drop
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...
Related questions
Question
![Run-1
Run-2
Run-3
Run-4
Average time(s) [H₂O2] (M) [I-](M)
210.6
74.3
314
82
Quantity
[Na₂S₂O3] stock
[KI] stock
[H₂O₂] stock
k'
0.04
0.04
0.0125
0.025
Value
0.005M
0.2M
0.1M
INITIAL CONCENTRATION
0.0386
0.04
0.08
0.1
0.1
Run 1
Run 2
Run 3
Run 4
Na₂S₂O3
0.005M
1 drop
1 drop
1 drop
1 drop
[S₂O3²- ] (M)
0.001
0.001
0.00125
0.00125
KI
0.1M
2 drops
KI
0.2M
2 drops
2 drops
2 drops
H₂O₂
0.05M
1 drop
Assuming that the colour change occurred at the moment the S₂03² was completely consumed,
determine the average rate of disappearance of S₂O3²- during this reaction (for Run #1):
From the rate of disappearance of S₂O3², determine the average rate of reaction for Run #1:
H₂O₂
0.1M
2 drops
2 drops
1 drop](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe31c5e57-f927-44e9-a19f-7b1a4337091e%2F29418c06-e3ba-42f0-aa88-3e3b239a458e%2Fv9kk7wc_processed.png&w=3840&q=75)
Transcribed Image Text:Run-1
Run-2
Run-3
Run-4
Average time(s) [H₂O2] (M) [I-](M)
210.6
74.3
314
82
Quantity
[Na₂S₂O3] stock
[KI] stock
[H₂O₂] stock
k'
0.04
0.04
0.0125
0.025
Value
0.005M
0.2M
0.1M
INITIAL CONCENTRATION
0.0386
0.04
0.08
0.1
0.1
Run 1
Run 2
Run 3
Run 4
Na₂S₂O3
0.005M
1 drop
1 drop
1 drop
1 drop
[S₂O3²- ] (M)
0.001
0.001
0.00125
0.00125
KI
0.1M
2 drops
KI
0.2M
2 drops
2 drops
2 drops
H₂O₂
0.05M
1 drop
Assuming that the colour change occurred at the moment the S₂03² was completely consumed,
determine the average rate of disappearance of S₂O3²- during this reaction (for Run #1):
From the rate of disappearance of S₂O3², determine the average rate of reaction for Run #1:
H₂O₂
0.1M
2 drops
2 drops
1 drop
![Part 1: Getting Ready
1. Obtain 5 pieces of filter paper from your TA
2. Record the exact stock concentrations of the reactants Into Table
2
3. Obtain one pump (10 mL) of NauSO; In a 50 ml beaker.
4. In a 50 mL beaker, obtain (12.5 mL) of 0.2 M K.
5. Obtain one pump (12.5 mL) of 0.1 M H₂O;in a 50mLbeaker and add 10
drops of GM HCL.
& Divide the filter paper into quarters
Part 2: Preparation of Solutions
1. Ina 25.00mL volumetric flask add one pump (12.5 mL) of 0.1MH₂O₂, add
10 drops of GM HCL and dilute to the mark with RO water.
2. In a 25.00 mL volumetric flask add one pump (12.5 mL) of 0.2M Kland dilute
to the mark with RO water.
Part 3: Run 1
1. Place your watch glass on top of your white bile
2. Place a piece of filter paper on top of a watch glass. Label the filter paper
with an X to mark the center or target area for your reagents (see Figure 1
on next page).
3. Add the reagents as shown in Table 1 on the target you marked on the filter
paper. Your medicine dropper should be no more than an inch from the
filter paper.
4. Start the time as soon as you add the first drop H₂O₂
5. Record the time when you see the first sight of brown on the filter paper.
6. Repeat steps 1-5 for this run four more times, cleaning the watch glass and
using a new filter paper for each trial.
Figure 1: Appearance of filter paper over time.
From left to right: Before reaction has started; first hint of brown appears too much brown (after the point time
should be recorded: an extreme example of brown
Run #
1
2
3
4
Trial 1 (s) Trial 2 (s) Trial 3 (s) Trial 4 (s) Trial 5 (s)
218
29
201 222 205
66 79
71
73 82.5
289 335 301 287 358
87
79
74 89 81
Objective
this experiment, you will use the method of initial rates to determine the rate law for an ledine clock reaction
Introduction
Kinetics and Pseudo-Order Conditions
and in pour
les
16-26 14.3
Ay
related to the reactant concentrations through an espression called the rate law for a particular reaction. For the
de clockreste studied in this experiment the gathe
- PIP
the reaction Chemperature depend
disk
Where
then you will strmine the value forkynd
that loneles
Since
oncentrations in order to manipulate the variation
large
Since the 1so much larger than the 11 and
effectively, while the relative changes in and the H0] are very large
neuro4
is possible but is much-eader if the parents are
ready combant value we will control the react
approximate a co
Where K-P
The comtatsudo-onder comtant-it behaves and can be treated an it were ante confor
rectant.
Reactions
[11
de creacically consist of two reactions occurring at the same time in a manner. The first
sslewation reaction which is the rate determining step. The second reaction reduction
Once the touring reed semed Reaction (4) can no longer prod
and the produced by Reaction begins to accurate in the system, showing acharacteristic yellow-brown
ckmeaction, an indicator such as starch or hidee is often added
change evide
we indicator, producing a deep black-blue colour Since this
happens very quickly once the thiosulphate is consumed the colour change is quite dramatic
Using a modification of the
of
I and HO, in the pudo rate laws. Rather than m
131
141
Method of initial Rates
ander to determine the rate law for the iodine dock studied the rate of the reaction with respect to the
pace will first be determined. This will be done by relating the time required for the appearance of
colour to be visible
to
By you com
ne the order of both
experient
erate for the reaction will follow the same trends in rate lng for a first onder reaction doubling the
loubles the ratel. The end reaction is taken as the moment
that is completely
and excess die begins to build up bee Reaction section below. In this method
Welco
the rate does not change the reaction
erate doubles huit heet
to
pletion, the action is 1" order with respe
the rates the e to completion, the reaction is 2erder with respect to us
emination for the order with respect to 10ound while Hus](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe31c5e57-f927-44e9-a19f-7b1a4337091e%2F29418c06-e3ba-42f0-aa88-3e3b239a458e%2F4x90wul_processed.png&w=3840&q=75)
Transcribed Image Text:Part 1: Getting Ready
1. Obtain 5 pieces of filter paper from your TA
2. Record the exact stock concentrations of the reactants Into Table
2
3. Obtain one pump (10 mL) of NauSO; In a 50 ml beaker.
4. In a 50 mL beaker, obtain (12.5 mL) of 0.2 M K.
5. Obtain one pump (12.5 mL) of 0.1 M H₂O;in a 50mLbeaker and add 10
drops of GM HCL.
& Divide the filter paper into quarters
Part 2: Preparation of Solutions
1. Ina 25.00mL volumetric flask add one pump (12.5 mL) of 0.1MH₂O₂, add
10 drops of GM HCL and dilute to the mark with RO water.
2. In a 25.00 mL volumetric flask add one pump (12.5 mL) of 0.2M Kland dilute
to the mark with RO water.
Part 3: Run 1
1. Place your watch glass on top of your white bile
2. Place a piece of filter paper on top of a watch glass. Label the filter paper
with an X to mark the center or target area for your reagents (see Figure 1
on next page).
3. Add the reagents as shown in Table 1 on the target you marked on the filter
paper. Your medicine dropper should be no more than an inch from the
filter paper.
4. Start the time as soon as you add the first drop H₂O₂
5. Record the time when you see the first sight of brown on the filter paper.
6. Repeat steps 1-5 for this run four more times, cleaning the watch glass and
using a new filter paper for each trial.
Figure 1: Appearance of filter paper over time.
From left to right: Before reaction has started; first hint of brown appears too much brown (after the point time
should be recorded: an extreme example of brown
Run #
1
2
3
4
Trial 1 (s) Trial 2 (s) Trial 3 (s) Trial 4 (s) Trial 5 (s)
218
29
201 222 205
66 79
71
73 82.5
289 335 301 287 358
87
79
74 89 81
Objective
this experiment, you will use the method of initial rates to determine the rate law for an ledine clock reaction
Introduction
Kinetics and Pseudo-Order Conditions
and in pour
les
16-26 14.3
Ay
related to the reactant concentrations through an espression called the rate law for a particular reaction. For the
de clockreste studied in this experiment the gathe
- PIP
the reaction Chemperature depend
disk
Where
then you will strmine the value forkynd
that loneles
Since
oncentrations in order to manipulate the variation
large
Since the 1so much larger than the 11 and
effectively, while the relative changes in and the H0] are very large
neuro4
is possible but is much-eader if the parents are
ready combant value we will control the react
approximate a co
Where K-P
The comtatsudo-onder comtant-it behaves and can be treated an it were ante confor
rectant.
Reactions
[11
de creacically consist of two reactions occurring at the same time in a manner. The first
sslewation reaction which is the rate determining step. The second reaction reduction
Once the touring reed semed Reaction (4) can no longer prod
and the produced by Reaction begins to accurate in the system, showing acharacteristic yellow-brown
ckmeaction, an indicator such as starch or hidee is often added
change evide
we indicator, producing a deep black-blue colour Since this
happens very quickly once the thiosulphate is consumed the colour change is quite dramatic
Using a modification of the
of
I and HO, in the pudo rate laws. Rather than m
131
141
Method of initial Rates
ander to determine the rate law for the iodine dock studied the rate of the reaction with respect to the
pace will first be determined. This will be done by relating the time required for the appearance of
colour to be visible
to
By you com
ne the order of both
experient
erate for the reaction will follow the same trends in rate lng for a first onder reaction doubling the
loubles the ratel. The end reaction is taken as the moment
that is completely
and excess die begins to build up bee Reaction section below. In this method
Welco
the rate does not change the reaction
erate doubles huit heet
to
pletion, the action is 1" order with respe
the rates the e to completion, the reaction is 2erder with respect to us
emination for the order with respect to 10ound while Hus
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