Kinetics of Hydrogen Peroxide

Topics: Rate equation, Reaction rate, Chemical kinetics Pages: 13 (3056 words) Published: March 17, 2008
Kinetics of Hydrogen Peroxide
February 22, 2007
Chem. 1130
TA: Ms. Babcock
Room 1830 Chemistry Annex

Kinetics of Hydrogen Peroxide

The major purpose of this experiment is to determine the rate law constant for the reaction of hydrogen peroxide and potassium iodide. In this experiment, the goal will be to try to measure the rate law constant at low acidity, since at low acidity, anything less than 1.0 x 10-3M, the effect of the hydrogen ion is negligible. To calculate the rate, the experiment will have to utilize the rate equation, which is expressed as Rate = k[H2O2]a[I-]b. At low acidity, the rate of the Hydrogen ion will not change, from our equation:

H2O2 (aq) + 2I- (aq) + 2H+ (aq) → I2 (aq) + 2H2O (l). Eqn. 1

If the rate in hydrogen does not change, it makes it easier to solve for the other rate constant. In this experiment, sodium thiosulfate will be added to suppress the rate of the reverse reaction. The objective is to measure the rate of the forward reaction. To do this, the rate of the reverse reaction must be eliminated. By using sodium thiosulfate accumulating Iodine on the left side and cause the reaction will be eliminated and it will cause the reaction to continue forward. Sodium thiosulfate will not react with any other compound in this solution, but will react rapidly and completely with iodine in the following way:

I2 (aq) + 2S2O32- → 2I- (aq) + S4O62- (aq)Eqn. 2

The rate constant can then be calculated from the forward reaction. This experiment will identify the rate constant from 5 solutions utilizing the above equation, only adding different concentrations of buffer, potassium iodide, starch, sodium thiosulfate, and hydrogen peroxide.

Kinetics of Hydrogen Peroxide

Before starting any step in this lab, five 250mL beakers must be obtained, cleaned, and dried. Also, this lab requires solutions of buffer, KI, starch, Na2S2O3, and H2O2. Other lab equipment to be used includes a stop watch and a thermometer.

After the beakers are cleaned, number the beakers one through five. Next, the five cleaned beakers will be used to prepare five different solutions from the following table:

Table: Concentrations for each solution in the experiment
Solution NumberBuffer0.300 M KIStarch0.0200 M Na2S2O3 Water0.100 M H2O2Total Volume 15.001.501.005.0082.505.00100.00

Take the beaker labeled #1 and add the ingredients for Solution # 1 in this order: buffer, KI, starch, and Na2S2O3. However, it is important that the H2O2 is added last! To add the hydrogen peroxide, find another 250mL beaker, clean it out, and pour the required concentration into the beaker. Then, once the other ingredients are added into the beaker marked Solution # 1, add the concentration of H2O2 and begin the timer. Mix the solution in Solution # 1 by pouring it into the H2O2 beaker and then back from the H2O2 beaker to the Solution # 1 repeatedly until the solution is well mixed. Then put Solution #1 on a white piece of paper and once the solution changes color, stop the stopwatch and record the reaction time. Next, rinse out the H2O2 beaker thoroughly and set it aside to be used for later. It is recommended to move along and prepare the other solutions in their designated beakers by following the same procedure listed here.

When the data has been collected, calculate the initial rate of reaction, the initial concentrations of H2O2 and I-, determine the correct rate equation, and calculate the average rate constant for the reaction.

This lab experiment will be performed by two members who will work together to carry out this lab.

For better detailed procedures and instructions, refer to the Chemistry Lab Book:

Kinetics of Hydrogen Peroxide CHEM 1130 Spring...
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