In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 5.00 mL 3.55 M acetone + 10.0 mL 1.80 M HCl + 10.0 mL 0.00600 M I2 + 25.0 mL H,O A student found that it took 354 seconds for the color of the I2 to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of I2 in the reaction mixture, [I2]o- Then use the equation A[12] Rate = - At t |M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H*, and iodine to I,. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). ORate Ok Om On Op O[Ace] O[H*]
In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 5.00 mL 3.55 M acetone + 10.0 mL 1.80 M HCl + 10.0 mL 0.00600 M I2 + 25.0 mL H,O A student found that it took 354 seconds for the color of the I2 to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of I2 in the reaction mixture, [I2]o- Then use the equation A[12] Rate = - At t |M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H*, and iodine to I,. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). ORate Ok Om On Op O[Ace] O[H*]
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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![In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture:
5.00 mL 3.55 M acetone + 10.0 mL 1.80 M HCl + 10.0 mL 0.00600 M I2 + 25.0 mL H,O
A student found that it took 354 seconds for the color of the I2 to disappear.
a. What was the rate of the reaction?
Hint: First find the initial concentration of I2 in the reaction mixture, [I2]o- Then use the equation
A[12]
Rate = -
At
t
|M/s
b. Write the rate equation.
(Abbreviate acetone to ace, H* ion to H*, and iodine to I,. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and
the order of reaction with respect to H* as p).
c. Select all the unknown variables in the equation in part (b).
ORate
Ok
Om
On
Op
O[Ace]
O[H*]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17b7c333-bc09-4ff0-9d99-0fb21b9f9655%2Fd6375f4d-5116-4fc3-aaf6-4c28481eabe6%2Fp0qbcp2k.png&w=3840&q=75)
Transcribed Image Text:In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture:
5.00 mL 3.55 M acetone + 10.0 mL 1.80 M HCl + 10.0 mL 0.00600 M I2 + 25.0 mL H,O
A student found that it took 354 seconds for the color of the I2 to disappear.
a. What was the rate of the reaction?
Hint: First find the initial concentration of I2 in the reaction mixture, [I2]o- Then use the equation
A[12]
Rate = -
At
t
|M/s
b. Write the rate equation.
(Abbreviate acetone to ace, H* ion to H*, and iodine to I,. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and
the order of reaction with respect to H* as p).
c. Select all the unknown variables in the equation in part (b).
ORate
Ok
Om
On
Op
O[Ace]
O[H*]
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