Rates of chemical reaction PDF

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Summary

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Description

Rates of chemical reaction Iodination of acetone

Jodyann Munroe

Purpose

To identify and measure the effects and rate of reactions, how it changes upon the time required for the reaction to occur, to determine the order of the reaction in relation to the reactant concentrations, to obtain the rate law, rate constant, and overall order for the chemical reaction.

Introduction Within a chemical reaction, time is a significant benefactor because it depicts how fast the reaction takes place. The rate of reactions was measured how quickly reactants were converted into products. Concentration as a big part to do with reactants. The reaction rate is found by observing the change in concentration of reactants or products over time; the unit that the change of concentration is measured in is molarity, in which time can either be counted in seconds or minutes depending on how fast the reaction occurs. In addition to concentration, the rate of the reaction does also depend on the addition of catalyst and temperature. The higher the temperature gets the more kinetic energy will be produced which will increase the chance of molecules collision allowing the products to form faster. This way determines the rate of chemical reaction that were conducted and observed from the experiments. Adjusting the concentration of reactants in each mixture and recording times of chemical reactions, we would be able to find the orders and the rate constant of the reaction, which then could be used to calculate the reaction rate, and the calculation of when the iodine was added to indicate the time of the reaction, and when the color changed.

Procedure `3 beakers were filled with approximately 40 mL of each solution. Into a flask, 10 mL of acetone

was added, with 10 mL of HCl, and 20 mL of water using the graduated cylinder. Add the stir bar and place on the magnetic stirrer. Start stirring the mixture. The graduate cylinder was rinsed out, and 10 mL of I2. I2 was poured into the flask and immediately start timing. When the color changed from yellow to clear, stop timing. The time was recorded how long it took to turn clear. Pour waste into the proper waste container. The process was repeated using the same amount of reactants.there more trails, twice each. One of the reactant volumes will be varied in each experiment. A given chart was followed. The rate of each reaction was determined using I2 initial concentration and the average time of each experiment. From the rates, the reaction was determined from each reactant. And finally, the rate constant each reaction trail.

Data

Trail

Acetone

HCl

I2

Water

Time 1

Time

Average

(mL)

(sec)

(sec)

time (sec)

1

10

10

10

20

88

82

85

2

5

10

10

25

170

174

172

3

10

5

10

25

180

160

170

4

10

10

5

25

42

44

43

Trail

Acetone

HCl

I2

Rate I2/average time

1

0.8M

0.20M

0.001M

1.176*10^-5

2

0.4M

..20M

0.001M

5.814*10^-6

3

..8M

.10M

0.001M

5.882*10^-6

4

.8M

.20M

0.0005M

1.63*10^-5

Trail

k

1

7.35*10^-5

2

72..675*10^-6

3

73.525*10^-6

4

10.1875

Calculations On a separate sheet of paper

Conclusions ‘Within this experiment, the reaction rate was determined. Different concentration of acetone and HCl was mixed and the times of the reaction when the color completely disappears and then calculated the reaction rate of each trial.

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