A second reaction mixture was made up in the following way: 2.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M I₂ + 1.0 mL H₂O What were the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture? [H] ini [12] ini [acetone]ini b. It took 140 seconds for the I2 color to disappear from the reaction mixture when it occurred at the same temperature as the reaction in Problem 2. M; What was the rate of the reaction? rate= M; Write Equation 3 as it would apply to the second reaction mixture: M c. Solve for the value of m, the order of the reaction with respect to acetone. (Use the logarithm method and calculate the value of m to two decimal places and then round to the nearest integer.)
A second reaction mixture was made up in the following way: 2.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M I₂ + 1.0 mL H₂O What were the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture? [H] ini [12] ini [acetone]ini b. It took 140 seconds for the I2 color to disappear from the reaction mixture when it occurred at the same temperature as the reaction in Problem 2. M; What was the rate of the reaction? rate= M; Write Equation 3 as it would apply to the second reaction mixture: M c. Solve for the value of m, the order of the reaction with respect to acetone. (Use the logarithm method and calculate the value of m to two decimal places and then round to the nearest integer.)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![1. In a reaction involving the iodination of acetone, the following volumes were used to
make up the reaction mixture.
1.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M 12+ 2.0 mL H₂O
a. Calculate the initial (diluted) concentration of acetone in the reaction mixture.
Moles =4.0.001
=0.004 moles
ImL
ЧМ
Moles (1+1+1+2) mL = 5mL
4=
0.004 mol
0.001
0.005 litre = 0.8M [acetone]ini = 0.8 M
b. Calculate the initial (diluted) concentration of the hydrogen ion, H+, in the reaction
mixture.
1.0.001 = 0.001 mol
0-001mole
0.005 Titre
=0-2M
[H*] ini = 0.2M
c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture.
1ml 0.005 M/₂
0.005-0.001= 5×10-6
6 moles
0.005 litre
5x10
= 0.0011
[12]ini = 0.001 M
2. Using the reaction mixture in Problem 1, a student found that it took 300 seconds for
the color of the 1₂ to disappear.
1
a. What was the rate of the reaction?
0.0050M 0.001L
50.600005 mol
10|p1+2) =5.0ml
rate=
0.001 M
300 S
0.000005
6.005
3.33·10-6m/s
0.0011
b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and 12 in
the reaction mixture, write Equation 3 as it would apply to the mixture.
Km (1₂) ^ (H+) P
=K (0.8)m (0.001) (0.2) P
c. What are the unknowns that remain in the equation in Part b?
к
3.33010-6
rate=
P](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5eb09660-693f-4b0a-9c98-8e645b8ba753%2Fb21bbf3f-5dc4-49a3-b83e-e0c360ebf5d0%2F74i653m_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. In a reaction involving the iodination of acetone, the following volumes were used to
make up the reaction mixture.
1.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M 12+ 2.0 mL H₂O
a. Calculate the initial (diluted) concentration of acetone in the reaction mixture.
Moles =4.0.001
=0.004 moles
ImL
ЧМ
Moles (1+1+1+2) mL = 5mL
4=
0.004 mol
0.001
0.005 litre = 0.8M [acetone]ini = 0.8 M
b. Calculate the initial (diluted) concentration of the hydrogen ion, H+, in the reaction
mixture.
1.0.001 = 0.001 mol
0-001mole
0.005 Titre
=0-2M
[H*] ini = 0.2M
c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture.
1ml 0.005 M/₂
0.005-0.001= 5×10-6
6 moles
0.005 litre
5x10
= 0.0011
[12]ini = 0.001 M
2. Using the reaction mixture in Problem 1, a student found that it took 300 seconds for
the color of the 1₂ to disappear.
1
a. What was the rate of the reaction?
0.0050M 0.001L
50.600005 mol
10|p1+2) =5.0ml
rate=
0.001 M
300 S
0.000005
6.005
3.33·10-6m/s
0.0011
b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and 12 in
the reaction mixture, write Equation 3 as it would apply to the mixture.
Km (1₂) ^ (H+) P
=K (0.8)m (0.001) (0.2) P
c. What are the unknowns that remain in the equation in Part b?
к
3.33010-6
rate=
P
![A second reaction mixture was made up in the following way:
2.0 mL 4.0 M acetone + 1.0 mL 1.0 M HC1 + 1.0 mL 0.0050 M I2 + 1.0 mL H₂O
a. What were the initial concentrations of acetone, H+ ion, and I2 in the reaction
mixture?
[acetone]ini
M; [H] ini
[12] ini
b. It took 140 seconds for the I2 color to disappear from the reaction mixture when it
occurred at the same temperature as the reaction in Problem 2.
C.
What was the rate of the reaction?
Write Equation 3 as it would apply to the second reaction mixture:
rate=
m
M;
Solve for the value of m, the order of the reaction with respect to acetone. (Use the
logarithm method and calculate the value of m to two decimal places and then round
to the nearest integer.)
(2 decimal places)
m
M
(nearest integer)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5eb09660-693f-4b0a-9c98-8e645b8ba753%2Fb21bbf3f-5dc4-49a3-b83e-e0c360ebf5d0%2Fab7n67g_processed.png&w=3840&q=75)
Transcribed Image Text:A second reaction mixture was made up in the following way:
2.0 mL 4.0 M acetone + 1.0 mL 1.0 M HC1 + 1.0 mL 0.0050 M I2 + 1.0 mL H₂O
a. What were the initial concentrations of acetone, H+ ion, and I2 in the reaction
mixture?
[acetone]ini
M; [H] ini
[12] ini
b. It took 140 seconds for the I2 color to disappear from the reaction mixture when it
occurred at the same temperature as the reaction in Problem 2.
C.
What was the rate of the reaction?
Write Equation 3 as it would apply to the second reaction mixture:
rate=
m
M;
Solve for the value of m, the order of the reaction with respect to acetone. (Use the
logarithm method and calculate the value of m to two decimal places and then round
to the nearest integer.)
(2 decimal places)
m
M
(nearest integer)
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