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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 ...
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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 I 2 , 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^ (I 2 )p^ , can be simplified to rate = k[I 2 ]/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 :
Procedure :
Data and Calculations:
I. Reaction Rate Data
Trial
Volume Acetone
Volume HCl
Volume Iodine
Volume H 2 O
Time 1 st^ Run
Time 2 nd^ Run
Average Time
1 5 mL 5 mL 5 mL 10 mL
2
3
4
5
III. Determination of the Rate Constant k
Trial 1
Trial 2
Trial 3
Trial 4
Average Value for k __________
IV. Prediction of Reaction Rate
Use the data from Trial 5 to compare actual and predicted rates of reaction.
Rate = k[acetone]m[I 2 ]n^ [H+^ ]p
[acetone] = __________ [I 2 ] = _________
[H+^ ] = _________ k(average) = _________
Predicted Rate = _______________ Experimental Rate = [I 2 ]/t = _______________
Questions:
and B. What happens to the rate if the concentrations of A and B are doubled?