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11 Dec 2019

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A student prepared the following mixtures and measured the time each took to react. Calculate the average time for each mixture (in seconds).

Mixture

Vol. of 4.0 M acetone (mL)

Vol. of 1.0 M HCl (mL)

Vol. of 0.0050 M I2 (mL)

Vol. of H2O (mL)

Time for Trial 1

Time for Trial 2

Average time (s)

1

10

10

10

20

249

251

250

2

20

10

10

10

123

125

124

3

10

20

10

10

121

124

122.5

4

10

10

5

25

124

126

125

To complete the following table:

Determine the initial concentration (molarity) of each reagent using the equation:

The Mstock and Vstock for each reagent are given in problem 1. The total volume is 50 mL for each trial.

Calculate the rate of the reaction using the equation

Mixture

[Acetone], M

[H+], M

[I2]0, M

Rate

1

0.80

0.20

0.0010

2

3

4

Determine the rate law by finding the orders of the reaction (m, n, and p).

Rate = k[acetone]m[H+]n[I2]p

Use the rate law determined in problem 3 to calculate the rate constant, k for each mixture. Find the average rate constant.

Mixture

1

2

3

4

Average

k

We will now consider reaction mixture 5. Calculate the molar concentrations of each reactant as done in problem 2.

4.0 M Acetone

1.0 M HCl

0.0050 M I2

H2O

Volume (mL)

10.0

5.0

10.0

25.0

Concentration (M)

--------------

Use the concentrations for Mixture 5 you just calculated, along with the orders of the reaction (m, n, and p, from problem 3), and the average rate constant (problem 4), to solve Eq. 2 for rate. This is a prediction of how long it will take for the I2 color to disappear from your mixture.

Rate = k[acetone]m[H+]n[I2]p

Predicted Rate:____________________

To find the predicted time, recall. Use the rate from problem 5 and the molar concentration of [I2]0 from problem 5 to solve for the predicted time.

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13 Dec 2019

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Related questions

In a reaction involving the iodination of acetone, the followingvolumes were used to make up the reaction mixture:

10 mL 4.0 M acetone + 10 mL 1.0 M HCl + 10 mL 0.0050 MI2, + 20 mL H20


2. Using the reaction mixture in Problem 1, a student found that ittook 250 seconds for the color of the I2, to disappear.

a. What was the rate of the reaction? Hint: First find the initialconcentration of I2 in the reaction mixture, [I2]. Then useEquation: rate=(delta(I2))/delta t) x(I2)0/t


rate = __________

b. Given the rate from Part a, and the initial concentrations ofacetone, H+ ion, and I2, in the reaction mixture, write Equation 3as it would apply to the mixture. Equation:rate=k(acetone)m(I2)n(H+)p

rate =

c. What are the unknowns that remain in the equation in Partb?

__________ __________ __________ __________

3. A second reaction mixture was made up in the followingway:

20 mL 4.0 M acetone + 10 mL 1.0 M HCl + 10 mL 0.0050 M I2 + 10 mLH,O

a. What were the initial concentrations of acetone, H+ ion, and I2,in the reaction mixture?



[acetone] __________ M; [H+] __________; [I2] __________ M




b. It took 120 seconds for the I2 color to disappear from thereaction mixture when it occurred at the same temperature as thereaction in Problem 2. What was the rate of the reaction?



rate __________ units __________

Write Equation 3 as it would apply to the second reaction mixture:equation: rate=k(acetone)m(I2)n(H+)p

rate =

c. Divide the equation in Part b by the equation in Problem 2b. Theresulting equation should have the ratio of the two rates on theleft side and a ratio of acetone concentrations raised to the mpower on the right. Write the resulting equation and solve for thevalue of m, the order of the reaction with respect to acetone.(Round off the value of m to the nearest integer.)



m = __________


4. A third reaction mixture was made up in the following way:

20 mL 4.0 M acetone + 10 mL 1.0 M HCl + 20 mL 0.0050 M I2,

If the reaction is zero order in I2, how long would it take for theI2, color to disappear at the tem¬perature of the reaction mixturein Problem 3?



__________ seconds

A student prepares a reaction mixture 1 by adding 10.0 mL of 4.0 M acetone, 10.0 mL of 1.0 M HCl , 10.0 mL of 0.0050 M I2, and 20.0 mL of water. The reaction mixture is initially yellow, but after 4 minutes and 22 seconds, the reaction mixture becomes clear indicating that the I2 has been completely consumed in the reaction. The student repeats the reaction (mixture 2) but instead of 10.0 mL of 4.0 M acetone he uses 20.0 mL of 4.0 M acetone and 10.0 mL of water rather than 20. The reaction goes to completion in 2 minutes and 10 seconds.

Acetone + I2 =====(HCl)=====> products

5. Assuming that all of the iodine is consumed in the reaction, what is the average rate of disappearance of I2 in M/s for reaction mixture 1?

6. In reaction mixture 2, the concentration of acetone was doubled and the concentration of I2 and HCl remained the same. What is the average rate of disappearance of I2 in M/s for reaction mixture 2?

7. Comparing the rates of reaction mixture 2 to the rate of reaction mixture 1, what is the exponent of the acetone in the general rate law?

) In a reaction involving the iodination of acetone, the followingvolumes were used to make up the reaction mixture:

10 ml 4.0 M acetone + 10 ml 1.0 M HCI + 10 ml 0.0050 M I2 + 20 mlH2O

A) How many moles of acetone were in the reaction mixture? Recallthat, for a component A, no. moles A=Ma* V, where Ma is themolarity of A and V is the volume in liters of the solution of Athat was used. ______________moles acetone

B) What was the molarity of acetone in the reaction mixture? Thevolume of the mixture was 50 ml, 0.0050 L, and the number of molesof acetone was found in part a. again.
M= no. moles A/ V of soln. in _________________M acetone
C) How could you double the molarity of the acetone in the reactionmixture, keeping the total volume at 50 ml and keeping the sameconcentration of H+ ion and I2 as in the original mixture?
A) you used 10 ml of 4 mole /1000ml soln
so you used
10ml*(4mole/1000ml)=0.04 moles

B) molarity in the total reaction mixture would be:

C)moles used/volume solution
= 0.04moles/(10ml + 10 ml + 10ml + 20 ml)*1000ml/liter
= 0.8M

2) Using the reaction mixture in Problem 1, a student found that ittook 250 seconds for the color of the I2 to disappear.



A) What was the rate of the reaction? Hint: first find the initialconcentration of I2 in the reaction mixture, (I2)0 then useequation 5

Rate =_____________



B) Given the rate from Part a, and the initial concentration ofacetone, H+ ion and I2 in the reaction mixture, write equation 3 asit would apply to the mixture.
rate+ k(acetone)m(I2)n(H+)p


Rate=

C) What are the unknowns that remain in the equation in partB?

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