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o0TEXASS Phan#137144DistribAll contents of the reaction flasks may be disposed of into the sink.al:lations:Aew the method of initial rates in yur text. You will need the values for the initial concentrations of each reactant asell as the rate.Hypothetical data for reaction: A+2B C+ 2DRun[Alo[BloInitial A[C]/At (Molarity/sec)10.150 M0.150 M8.0020.150 M0.300 M16.030.300 MRate = k[A]* [B]. We need to calculate x, y and k0.150 M32.0To get x, we have to hold [B] constant and just see how [A] affects the rate. Take the ratio of Run 3/Run 1Run 3Initial ΔΙCI/ΔtInitial A[C]/At32.0 M/sec8.0 M/seck[Al[B]Yk[A]* [B]Yk(0.300M)x (0.150M)k(0.150M)* (0.150 M)XRun 1YSimplifying:4.0 (0.150M) * / (0.150M) *4.0 (0.300/0.150)x or 4.0 = 2* Or x 2orDo the same for B (holding [A] constant) and discover that y = 1.You can calculate k as well. Using run 1:8.00 M/sec k (0.150M)1 (0.150M)1and solving for k, we get k = 356 M1 s1'k' can be calculated using any of the three runs from Part IFor your data:Find x and y as explained above. Calculate k for each run and average the three values at the end. If your values for xand y do not turn out to be whole numbers, round to the nearest whole number. Write the Rate Law using your valuesfor x, y and k:= k [IF]* [H2O2]'Rate CVSOSAGCa20ou ud SreTEXAS INSTRUMENTSDistribjock Reaction Part 1: PostLabNameUsing your calcuations from your pre-lab, how many moles of S2O3 are consumed in the experiment?=cocoz5 mol s203300.OIOM S203=M9rYol sz OO023 LS4O62(aq). How many moles of 12 will react with the 2YI2. Given that: 2 (aq) + 2 S2O32(aq)21 (aq).25L2-S 1a s.2.S adOmoles of S2O32-?mol szoe?M:molesZmo1s203moiesMxLCalculate the molarity of l2 that reacted [All: (divide moles reacted by total reaction volume) (42.5mL)3./.0425) L(1.25x 10Smo)2.94x 10ALT2JFill in the initial concentrations below using the chart on your pre-lab.4.Reaction Rate (in Ms)= [Al2 ] / At2.94 x IO- M AI2Reaction Time (in s)Initial [ IT MInitial [H2O2]MRunTemp(°C)At3प S34 S8.65 x loZ1.3 c.0176M0116121.lc0196-00882S S452L0- MsTCA1232.94X10-421.1 C .008%१ ८c017036 ५ s10-6 Ms-Show calculations for x and y: (Include appropriate units, attacha separate sheet if necessary.)5.fateraterate28. SA1O6MS-Rate = K CA LBYYoe 3raHeRare -K CIrate 3H202V(E(round to the nearest whole number)y=

Question

I need help finding x and y using my data and the equation shown in the image. I did the work but I wanted to verify if it was right. The second image has the data I need to use in order to fondness x and y. I need help with question #5. 

o0
TEXAS
S Phan
#137144
Distrib
All contents of the reaction flasks may be disposed of into the sink.
al:
lations:
Aew the method of initial rates in yur text. You will need the values for the initial concentrations of each reactant as
ell as the rate.
Hypothetical data for reaction: A+2B C+ 2D
Run
[Alo
[Blo
Initial A[C]/At (Molarity/sec)
1
0.150 M
0.150 M
8.00
2
0.150 M
0.300 M
16.0
3
0.300 M
Rate = k[A]* [B]. We need to calculate x, y and k
0.150 M
32.0
To get x, we have to hold [B] constant and just see how [A] affects the rate. Take the ratio of Run 3/Run 1
Run 3
Initial ΔΙCI/Δt
Initial A[C]/At
32.0 M/sec
8.0 M/sec
k[Al[B]Y
k[A]* [B]Y
k(0.300M)x (0.150M)
k(0.150M)* (0.150 M)
X
Run 1
Y
Simplifying:
4.0 (0.150M) * / (0.150M) *
4.0 (0.300/0.150)x or 4.0 = 2* Or x 2
or
Do the same for B (holding [A] constant) and discover that y = 1.
You can calculate k as well. Using run 1:
8.00 M/sec k (0.150M)1 (0.150M)1
and solving for k, we get k = 356 M1 s1
'k' can be calculated using any of the three runs from Part I
For your data:
Find x and y as explained above. Calculate k for each run and average the three values at the end. If your values for x
and y do not turn out to be whole numbers, round to the nearest whole number. Write the Rate Law using your values
for x, y and k:
= k [IF]* [H2O2]'
Rate
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o0 TEXAS S Phan #137144 Distrib All contents of the reaction flasks may be disposed of into the sink. al: lations: Aew the method of initial rates in yur text. You will need the values for the initial concentrations of each reactant as ell as the rate. Hypothetical data for reaction: A+2B C+ 2D Run [Alo [Blo Initial A[C]/At (Molarity/sec) 1 0.150 M 0.150 M 8.00 2 0.150 M 0.300 M 16.0 3 0.300 M Rate = k[A]* [B]. We need to calculate x, y and k 0.150 M 32.0 To get x, we have to hold [B] constant and just see how [A] affects the rate. Take the ratio of Run 3/Run 1 Run 3 Initial ΔΙCI/Δt Initial A[C]/At 32.0 M/sec 8.0 M/sec k[Al[B]Y k[A]* [B]Y k(0.300M)x (0.150M) k(0.150M)* (0.150 M) X Run 1 Y Simplifying: 4.0 (0.150M) * / (0.150M) * 4.0 (0.300/0.150)x or 4.0 = 2* Or x 2 or Do the same for B (holding [A] constant) and discover that y = 1. You can calculate k as well. Using run 1: 8.00 M/sec k (0.150M)1 (0.150M)1 and solving for k, we get k = 356 M1 s1 'k' can be calculated using any of the three runs from Part I For your data: Find x and y as explained above. Calculate k for each run and average the three values at the end. If your values for x and y do not turn out to be whole numbers, round to the nearest whole number. Write the Rate Law using your values for x, y and k: = k [IF]* [H2O2]' Rate

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CVSO
SAG
Ca
2
0
ou ud Sre
TEXAS INSTRUMENTS
Distrib
jock Reaction Part 1: PostLab
Name
Using your calcuations from your pre-lab, how many moles of S2O3 are consumed in the experiment?
=cocoz5 mol s203
300
.OIOM S203=M9
rYol sz O
O023 L
S4O62(aq). How many moles of 12 will react with the 2
YI
2. Given that: 2 (aq) + 2 S2O32(aq)
21 (aq)
.25
L2-S 1a s.
2.S adO
moles of S2O32-?
mol szoe?
M:moles
Zmo1s203
moiesMxL
Calculate the molarity of l2 that reacted [All: (divide moles reacted by total reaction volume) (42.5mL)
3.
/.0425) L
(1.25x 10Smo)
2.94x 10
ALT2J
Fill in the initial concentrations below using the chart on your pre-lab.
4.
Reaction Rate (in Ms)
= [Al2 ] / At
2.94 x IO- M AI2
Reaction Time (in s)
Initial [ IT M
Initial [H2O2]M
Run
Temp(°C)
At
3प S
34 S
8.65 x lo
Z1.3 c.0176M0116
1
21.lc
0196-0088
2
S S
452
L0- MsT
CA123
2.94
X10-4
21.1 C .008%
१ ८c
0170
3
6 ५ s
10-6 Ms-
Show calculations for x and y: (Include appropriate units, attacha separate sheet if necessary.)
5.
fate
rate
rate2
8. SA1O6MS-
Rate = K CA LBY
Yoe 3
raHe
Rare -K CI
rate 3
H202
V(E
(round to the nearest whole number)
y=
help_outline

Image Transcriptionclose

CVSO SAG Ca 2 0 ou ud Sre TEXAS INSTRUMENTS Distrib jock Reaction Part 1: PostLab Name Using your calcuations from your pre-lab, how many moles of S2O3 are consumed in the experiment? =cocoz5 mol s203 300 .OIOM S203=M9 rYol sz O O023 L S4O62(aq). How many moles of 12 will react with the 2 YI 2. Given that: 2 (aq) + 2 S2O32(aq) 21 (aq) .25 L2-S 1a s. 2.S adO moles of S2O32-? mol szoe? M:moles Zmo1s203 moiesMxL Calculate the molarity of l2 that reacted [All: (divide moles reacted by total reaction volume) (42.5mL) 3. /.0425) L (1.25x 10Smo) 2.94x 10 ALT2J Fill in the initial concentrations below using the chart on your pre-lab. 4. Reaction Rate (in Ms) = [Al2 ] / At 2.94 x IO- M AI2 Reaction Time (in s) Initial [ IT M Initial [H2O2]M Run Temp(°C) At 3प S 34 S 8.65 x lo Z1.3 c.0176M0116 1 21.lc 0196-0088 2 S S 452 L0- MsT CA123 2.94 X10-4 21.1 C .008% १ ८c 0170 3 6 ५ s 10-6 Ms- Show calculations for x and y: (Include appropriate units, attacha separate sheet if necessary.) 5. fate rate rate2 8. SA1O6MS- Rate = K CA LBY Yoe 3 raHe Rare -K CI rate 3 H202 V(E (round to the nearest whole number) y=

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check_circleAnswer
Step 1

It is required to calculate the value of x and y for the following rate law expression which is,

Rate k [IH2O02]*
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Rate k [IH2O02]*

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Step 2

The given data is as follows,

I
H2O2
Rate
8.65 x 10-6
4.52 x 10-6
0.0176
0.0176
0.0176
0.0088
4.60 x 10-6
0.0088
0.0176
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I H2O2 Rate 8.65 x 10-6 4.52 x 10-6 0.0176 0.0176 0.0176 0.0088 4.60 x 10-6 0.0088 0.0176

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Step 3

To calculate the value of x, it is required to fix the concentration of H2O2 hence for 1st and 3rd run ...

k [I]*H202
k [I-]*H202]
Rate 1
Rate 3
(0.0176
X
8.65 x 10-6
4.60 x 10-6
0.0088.
1.88 2
log (1.88) x log (2)
x= 0.91
help_outline

Image Transcriptionclose

k [I]*H202 k [I-]*H202] Rate 1 Rate 3 (0.0176 X 8.65 x 10-6 4.60 x 10-6 0.0088. 1.88 2 log (1.88) x log (2) x= 0.91

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