Kinetics of Hydrogen Peroxide
Kinetics of Hydrogen Peroxide
February 22, 2007
Chem. 1130
TA: Ms. Babcock
Room 1830 Chemistry Annex
PURPOSE OF THE EXPERIMENT
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.
PROCEDURES TO BE USED
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
February 22, 2007
Chem. 1130
TA: Ms. Babcock
Room 1830 Chemistry Annex
PURPOSE OF THE EXPERIMENT
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.
PROCEDURES TO BE USED
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