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 0.001 (1+1+112) mL 4= 0.004 mol 0.005 Titre =0.8 [acetonelini = 0.8M b. Calculate the initial (diluted) concentration of the hydrogen ion, H*, in the reaction mixture. 1.0.001 = 0-001 mole 0.005 Titre =0.2M = 5mL 0.001 mol [H]ini = 0.2M c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture. Iml 0.005M/2 0.005 0.001 = 5×10-6 5x10 moles 0.005 litre rate= = 0.001M [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. a. What was the rate of the reaction? rate= 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. c. What are the unknowns that remain in the equation in Part b?
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 0.001 (1+1+112) mL 4= 0.004 mol 0.005 Titre =0.8 [acetonelini = 0.8M b. Calculate the initial (diluted) concentration of the hydrogen ion, H*, in the reaction mixture. 1.0.001 = 0-001 mole 0.005 Titre =0.2M = 5mL 0.001 mol [H]ini = 0.2M c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture. Iml 0.005M/2 0.005 0.001 = 5×10-6 5x10 moles 0.005 litre rate= = 0.001M [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. a. What was the rate of the reaction? rate= 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. c. What are the unknowns that remain in the equation in Part b?
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Question
Please help with the second problem, the first is already done
![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 mole s
ImL
4 M.
Moles (1+1+112) mL = 5mL
0.004 mol
0.001
41=
0.005 Titre = 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
0-001 mole
0.005 Titre
-0.2M
[H*]ini = 0.2M
c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture.
Iml
0.005M/2
0.005 0.001 = 5×10-6
5 x 10-6 moles
0.005 litre
= 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.
a. What was the rate of the reaction?
T
rate=
rate=
b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and I₂ in
the reaction mixture, write Equation 3 as it would apply to the mixture.
c. What are the unknowns that remain in the equation in Part b?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5eb09660-693f-4b0a-9c98-8e645b8ba753%2Fb08a7c8d-e330-4357-880c-74f0bda08920%2Fg6lt6rl_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 mole s
ImL
4 M.
Moles (1+1+112) mL = 5mL
0.004 mol
0.001
41=
0.005 Titre = 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
0-001 mole
0.005 Titre
-0.2M
[H*]ini = 0.2M
c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture.
Iml
0.005M/2
0.005 0.001 = 5×10-6
5 x 10-6 moles
0.005 litre
= 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.
a. What was the rate of the reaction?
T
rate=
rate=
b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and I₂ in
the reaction mixture, write Equation 3 as it would apply to the mixture.
c. What are the unknowns that remain in the equation in Part b?
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