Measuring the rate of reaction

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MEASURING RATE OF THE REACTION OF YOUR CHOICE

Research question: what is the rate of change of the reaction of decomposition of hydrogen peroxide using different amounts of different catalysts?

Aim: to learn what effect do different amounts of biological catalyst liver and chemical catalyst MnO2 have on the rate of change of the reaction of decomposition of hydrogen peroxide.

Hypothesis: we believe that the more catalyst is added, the faster the rate of reaction will be. It is also expected that MnO2 will be a better catalyst than the biological one i.e. liver.

The equipment:                                  The substances:

Graduated tube        water

Clamp stand        manganese oxide (MnO2)

Water through                                       1M hydrogen peroxide (H2O2)

Delivery tube        liver

Stopper        

Conical flask

Stop watch

The method:

The reaction of decomposition of hydrogen peroxide is as follows:

2H2O2 (l)      2H2O(l)  + O2(g)

The rate of reaction will be calculated with reference to the amount of oxygen gases obtained. The amount of oxygen gases will be obtained using the process of displacement of water by O2 gases. The procedure is the following:

  1. The apparatus (Picture 1.) is constructed for collecting the O2 gases.
  2. The water through and the graduated tube are filled with water.
  3. 10 ml of H2O2 is poured in the conical flask.
  4. 0.2 g of MnO2 is added to the flask.
  5. The stopwatch is started immediately and the amount of O2 in the graduated tube is recorded every 10 seconds for around 80 seconds.
  6. Steps 2-5 are repeated another time with different amount of MnO2 : 0.1 g.
  7. Steps 2-5 are repeated 3 times with different amounts of liver as catalyst: 0.2g, 0.1 g.
  8. The results are considered to obtain the rates of reactions.
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Data collection and processing:

Table 1. The volume of O2 (ml) using MnO2 as a catalyst

Table 2. The volume of O2 (ml) using liver as a catalyst

The uncertainties of a mass of catalyst are +-0.05 g and the uncertainties of the volume of O2 are      +-0.1 ml, the uncertainties of time are +-0.1 s.

Below the results obtained are represented graphically:

Rate of reaction = increase in concentration of product ∕ time

2H2O2 (l)     2H2O(l)  + O2(g)

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