Effect of Catalysts on Rate of Reaction
This practical lesson covers:
- The effects of catalysts on the decomposition of hydrogen peroxide
Investigating the effect of catalysts on rates of reaction
Aim
To investigate the effects of various catalysts on the decomposition of hydrogen peroxide.
Background information
Catalysts speed up chemical reactions without being consumed. They lower the activation energy, providing an alternative pathway for the reaction. In this practical, you'll investigate how different catalysts—manganese (IV) oxide, platinum, iron (V) oxide, and vanadium (V) oxide, affect the rate of decomposition of hydrogen peroxide. The effectiveness of each catalyst will be assessed by measuring the volume of oxygen gas produced over time using a gas syringe.
Equipment
- Conical flask
- Gas syringe
- Bung and delivery tube
- Measuring cylinder
- Digital mass balance
- Timer
- Hydrogen peroxide
- Manganese (IV) oxide
- Platinum
- Iron (V) oxide
- Vanadium (V) oxide
Method
- Using a measuring cylinder, measure 60 cm3 of hydrogen peroxide and pour it into the conical flask.
- Connect the gas syringe to the delivery tube.
- Measure 0.75 g of the first catalyst.
- Place the first catalyst in the hydrogen peroxide and immediately attach the bung to the conical flask. Start the timer.
- Measure the amount of gas in the syringe every 10 seconds for 1 minute.
- Repeat steps 1-5 with all catalysts being tested.
What is the effect of catalysts on the decomposition of hydrogen peroxide?
catalysts slow down the reaction.
catalysts speed up the reaction.
catalysts do not affect the rate of reaction.
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How do catalysts work in chemical reactions?
they are consumed in the reaction.
they provide an alternative pathway for the reaction.
they increase the activation energy.
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What happens to the catalyst at the end of the reaction?
it is used up.
it remains unchanged.
it is transformed into a different substance.
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