Iodination of Acetone 2
Rates of Reaction: Iodination of Acetone
Introduction:
The rate at which a chemical reaction occurs depends on several factors: the nature of the reaction, the concentrations of the reactants, the temperature, and the presence of possible catalysts. In this experiment you will study the kinetics of the reaction between iodine and acetone in acid solution:
For this reaction, you will determine the order of the reaction with respect to acetone and HCl and find a value for the rate constant, k. Since the concentrations of acetone and HCl are much higher than that of I2, the concentrations of acetone and HCl will change very little. Thus the rate will be determined by the time needed for iodine to be used up. Iodine has color so you can easily follow changes in iodine concentration visually. The equation, rate = k(A)m(H+)n(I2)p, can be simplified to rate = k[I2]/t since the values for acetone and HCl essentially remain constant during the course of any run.
Purpose:
The purpose of this reaction is to determine the orders for the reactants, the rate expression, and the rate constant for the reaction between iodine and acetone.
Equipment/Materials:
4.0 M acetone solution 125 mL Erlenmeyer flasks 1.0 M HCl solution 10 mL graduated cylinders 0.0050 M iodine solution watch or other timing device 100 mL beakers watch glass covers for beakers
Safety:
Always wear an apron and goggles in the lab
Acetone is flammable. There should be no open flames in the room.
Procedure:
1. Fill in the volumes in Data Table 1 for Trials 2 -- 4. Double the volume of only one reagent at a time, and use the water to maintain a constant total volume. (Volumes for Trial 5 will be determined once data on the preceding trials has been collected.)
2. For Trial 1, pipet the appropriate amount of actone, HCl, and water; the iodine must be added last. (Be sure to use the correct pipet tip for each liquid.)
3. Simultaneously add the iodine and start the stopwatch;
Introduction:
The rate at which a chemical reaction occurs depends on several factors: the nature of the reaction, the concentrations of the reactants, the temperature, and the presence of possible catalysts. In this experiment you will study the kinetics of the reaction between iodine and acetone in acid solution:
For this reaction, you will determine the order of the reaction with respect to acetone and HCl and find a value for the rate constant, k. Since the concentrations of acetone and HCl are much higher than that of I2, the concentrations of acetone and HCl will change very little. Thus the rate will be determined by the time needed for iodine to be used up. Iodine has color so you can easily follow changes in iodine concentration visually. The equation, rate = k(A)m(H+)n(I2)p, can be simplified to rate = k[I2]/t since the values for acetone and HCl essentially remain constant during the course of any run.
Purpose:
The purpose of this reaction is to determine the orders for the reactants, the rate expression, and the rate constant for the reaction between iodine and acetone.
Equipment/Materials:
4.0 M acetone solution 125 mL Erlenmeyer flasks 1.0 M HCl solution 10 mL graduated cylinders 0.0050 M iodine solution watch or other timing device 100 mL beakers watch glass covers for beakers
Safety:
Always wear an apron and goggles in the lab
Acetone is flammable. There should be no open flames in the room.
Procedure:
1. Fill in the volumes in Data Table 1 for Trials 2 -- 4. Double the volume of only one reagent at a time, and use the water to maintain a constant total volume. (Volumes for Trial 5 will be determined once data on the preceding trials has been collected.)
2. For Trial 1, pipet the appropriate amount of actone, HCl, and water; the iodine must be added last. (Be sure to use the correct pipet tip for each liquid.)
3. Simultaneously add the iodine and start the stopwatch;