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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Question
I just need to know if all my work/calculations with this lab report are correct, thank you so much!
![How measure the rate? I2 is yellow. Will measure how long
for it to react (lose its color).
So, Rate = A[l2]/Atime
Data and Calculations:
Table 1. Reactant Volumes & Reaction Times
Volume (ml) of:
Mixture
4.0 M
acetone
1.0 M
HCI
time (sec)
0.0050 M
H20
12
A
B
1.00
1.00
230
1.00
1.00
1.00
2.00
1.00
2.00
1.00
106
120
110
1.00
2.00
1.00
1.00
1.00
0.50
2.50
Table 2. Initial Concentrations & Rate of Reaction
Mixture
A
B
[acetone]
.80 M
[H*]
.20 M
[k]
.0010 M
Rate =A[la]/time
4.34 x 10-6
9.43 x 10 -6
1.6 M
.80M
•20M
0010M
.0010 4
0005M
8.33 x 10-6
4.54 x lo-G
.40M
D
• 80 M
- 20 M
The Dilution Factor Method:
Original V
(4M)(1 ml) = .8M
(5 ml)
Final Total V
Reactant Order Determination
Calculate the value of m (order with respect to acetone)
1.6
0.000009433
2= 2.17
Rates = k[ace]m[ÁT
Ratea = k[ace]™[H]
0.8
0.000004347
1.12
(2 decimals) m=,
(nearest whole number)
m =
Calculate the value of n (order with respect to the H*)
0.000008 333
Rate C
.40
2 = 1.92
Rate A
· 20
0.000004347
_0.94
(2 decimals) n=
(nearest whole number)
Calculate the value of p (order with respect to the l2)
Experiments AtD 0.0005
0.000004545
0.000004347
0.5M: 1,04
0.0010
p=-0.06
(2 decimals) p=
(nearest whole number)
Write the overall Rate Law: Rate = k[acetone]( D[H*j( \ >[lz](O)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17525826-644e-4b54-80a2-4cc5c7d853ae%2Fafc5cdab-7d0f-497c-9589-81d0b70fe3b1%2Fsl8zg4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:How measure the rate? I2 is yellow. Will measure how long
for it to react (lose its color).
So, Rate = A[l2]/Atime
Data and Calculations:
Table 1. Reactant Volumes & Reaction Times
Volume (ml) of:
Mixture
4.0 M
acetone
1.0 M
HCI
time (sec)
0.0050 M
H20
12
A
B
1.00
1.00
230
1.00
1.00
1.00
2.00
1.00
2.00
1.00
106
120
110
1.00
2.00
1.00
1.00
1.00
0.50
2.50
Table 2. Initial Concentrations & Rate of Reaction
Mixture
A
B
[acetone]
.80 M
[H*]
.20 M
[k]
.0010 M
Rate =A[la]/time
4.34 x 10-6
9.43 x 10 -6
1.6 M
.80M
•20M
0010M
.0010 4
0005M
8.33 x 10-6
4.54 x lo-G
.40M
D
• 80 M
- 20 M
The Dilution Factor Method:
Original V
(4M)(1 ml) = .8M
(5 ml)
Final Total V
Reactant Order Determination
Calculate the value of m (order with respect to acetone)
1.6
0.000009433
2= 2.17
Rates = k[ace]m[ÁT
Ratea = k[ace]™[H]
0.8
0.000004347
1.12
(2 decimals) m=,
(nearest whole number)
m =
Calculate the value of n (order with respect to the H*)
0.000008 333
Rate C
.40
2 = 1.92
Rate A
· 20
0.000004347
_0.94
(2 decimals) n=
(nearest whole number)
Calculate the value of p (order with respect to the l2)
Experiments AtD 0.0005
0.000004545
0.000004347
0.5M: 1,04
0.0010
p=-0.06
(2 decimals) p=
(nearest whole number)
Write the overall Rate Law: Rate = k[acetone]( D[H*j( \ >[lz](O)
![Determination of the Rate Constant, k
mixture
A
В
C
D
average
2.71 x 10-5 2.94 x 10-5 2.60x1o-5 2.84 x 10 -52.76x10-5
k
Example: Ratea = k[ace]m[H*]*[l2]° klace]'C H+]' [l2]°
%3D
A :4.34x 10-6
(0.80)'CO.20)'CO.0010)0
= 2.71 x 10-5
B: 9.43 x 10-6
(1.6)'L0.20)' Co.0010)°
= 2.94 x10:5
C: 8. 33 x 10-6
= 2.60 x lo-5
Co.80)'CO.40)'CO.0010)0
D: 4.54 x1o - C
= 2.84 X10- 5
Co.80)'C0.20)' C0.0005)0
Prediction of a Reaction Rate
Use
your average k and these concentrations to predict the reaction rate.
[acetone] = 1.2 M, [H*] = .15 M, [l2] = .002 M
%3D
Rate =
2.76 x 16-5(1.2)'(o.15)'C0.002)° = 4.97 x10-6
0.002M
- 402 seconds
Therefore, Atime = All2]
Rate
Rate = All2]
4.97x10-6
Atime
Use this last equation to predict how long, in seconds,
it will take for the l2 to disappear.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17525826-644e-4b54-80a2-4cc5c7d853ae%2Fafc5cdab-7d0f-497c-9589-81d0b70fe3b1%2F72chv6o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Determination of the Rate Constant, k
mixture
A
В
C
D
average
2.71 x 10-5 2.94 x 10-5 2.60x1o-5 2.84 x 10 -52.76x10-5
k
Example: Ratea = k[ace]m[H*]*[l2]° klace]'C H+]' [l2]°
%3D
A :4.34x 10-6
(0.80)'CO.20)'CO.0010)0
= 2.71 x 10-5
B: 9.43 x 10-6
(1.6)'L0.20)' Co.0010)°
= 2.94 x10:5
C: 8. 33 x 10-6
= 2.60 x lo-5
Co.80)'CO.40)'CO.0010)0
D: 4.54 x1o - C
= 2.84 X10- 5
Co.80)'C0.20)' C0.0005)0
Prediction of a Reaction Rate
Use
your average k and these concentrations to predict the reaction rate.
[acetone] = 1.2 M, [H*] = .15 M, [l2] = .002 M
%3D
Rate =
2.76 x 16-5(1.2)'(o.15)'C0.002)° = 4.97 x10-6
0.002M
- 402 seconds
Therefore, Atime = All2]
Rate
Rate = All2]
4.97x10-6
Atime
Use this last equation to predict how long, in seconds,
it will take for the l2 to disappear.
Expert Solution
Step 1
The above kinetics experiment, iodination of acetone by initial rate method is a overall second order reaction.
The order with respect to acetone and Hydrogen ion is first. however the order with respect to iodine is zero.
All the given calculation are correct.
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