Decomposition Lab

D0ecomposition of Hydrogen Peroxide Lab

Introduction:

Hydrogen Peroxide (2H2O2) is a weak acid, that is both odourless and colourless, however it acts a powerful bleaching agent. It has many uses such as acting as a disinfector, oxidiser and antiseptic, etc.

The decomposition of hydrogen peroxide always results in water and oxygen (as seen below)

2H2O2(aq) --> 2H2O(l) + O2(g)

However, independantly it's rate of reaction is quite slow and it would take a significant amount of time to note an changes in the process. Consequently, many scientist use catalysts to speed up the process. These catalysts are usually transitional metals or enzymes. Each catalyst has a different effect on the original solution.

In order to investigate the process of the decomposition of hydrogen peroxide, two different catalysts were used - Manganese Dioxide (MnO2) and Potassium Iodide (KI). The molar concentration of these catalysts are 0.5 M. The amount of the hydrogen peroxide soluntion will remain constant during the expirement, however the concentration of hydrogen peroxide in the solutions will differ between 2% and 4%.

A titration method will be used in order to determine the amount of Manganese Dioxide and Potassium Iodide needed in order to cause a noticable reaction with the hydrogen peroxide.

The pressure of ...

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A titration method will be used in order to determine the amount of Manganese Dioxide and Potassium Iodide needed in order to cause a noticable reaction with the hydrogen peroxide.

The pressure of the reaction will be recorded throughout the expirement to calculate how the catalysts affect the reaction by measuring the amount of oxygen released, hence determining the affects of different catalysts and concentrations of the process.

Purpose:

How do two different catalysts (manganese dioxide and potassium iodide) affect the rate of reaction in decomposing two different molar concentration (2% and 4%) solutions of hydrogen peroxide.

Variables:

Independant: The catalyst used (MnO2 or KI) and the concentration of the hydrogen peroxide (2% and 4%)

Dependent: The amount of the catalyst needed in order to cause a noticable reaction and the amount of oxygen released, hence the amount of pressure.

Controlled: The molar concentration of the two catalysts and the amount of hydrogen peroxide.

Materials:

Flasks
2% 2H2O2 (30 ml)
4% 2H2O2 (30 ml)
0.5 M MnO2
0.5 M KI
1 Lab Pro, (or sensor collector)
1 Pressure sensor reader
Burette with stand
Eye dropper
2 test tubes

Hypothesis:

As the concentration of the hydrogen solution increases, more amount of the catalysts will be required to produce a noticable reaction, hence more oxygen will be produced. 75]

Procedure:

Step 1: Pour 15 ml of the 2% hydrogen peroxide into 2 test tubes, and label one as 2% 2H202 - MnO2 and label the other on as 2% 2H202 - KI

Step 2: Complete Step # 1, however substitute the 2% with 4%

Step 3: Step up Lab Pro and Pressure Sensor

Step 4: Set up the titration (burette, clamp and stand)

Step 5: Pour the manganese dioxide into the burette and place the 2% - MNO2 test tube under the burette and titrate the catalyst into the test tube, while reading the pressure.

Step 6: Record the pressure as the reaction bubbles out

Step 7: Repeat the date for 4 % 2H2O2 and as well as the KI for both 2% 2H2O2 and the 4% 2H2O2.

Step 8: Record the 0results in a table and conclude and analyze the data.