Try this: Super yeast
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You will need these materials. |
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Add 1/2 cup of hydrogen peroxide, a squirt of detergent and a few drops of food colouring to the bottle. |
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Dissolve the yeast in warm water. |
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Add the yeast mixture to the bottle and observe. |
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Safety: This activity uses hydrogen peroxide which can cause irritation. Read any safety instructions. Do not consume the chemicals used and wash your hands after completing the activity. See the CSIRO Education safety page for more information.
You will need
- Safety glasses
- Plastic bottle
- Hydrogen peroxide (available in pharmacies)
- Yeast
- Funnel
- Detergent
- Measuring cup
- Measuring spoons
- Food colouring
- Warm water
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Tray
What to do
- Put on the safety glasses.
- Place the bottle in the tray and add ½ cup of hydrogen peroxide.
- Add a squirt of detergent and a few drops of food colouring.
- Dissolve 1 teaspoon of yeast in 2 tablespoons of warm water.
- Add the yeast and water mixture to the bottle. What do you observe?
What's happening?
Hydrogen peroxide undergoes the following decomposition reaction:
2H2O2(l) → 2H2O(l) + O2(g)
Hydrogen peroxide (liquid) → water (liquid) + oxygen (gas)
Under normal circumstances this reaction happens slowly, with no obvious visible reaction taking place.
Chemical reactions need some energy such as light or heat to start. The amount of energy required to initiate a chemical is called the activation energy. In the reaction above, the activation energy is relatively high, so the reaction proceeds slowly.
Yeast is a microorganism that produces an enzyme called catalase. Catalase lowers the activation energy for the decomposition of hydrogen peroxide. The lower activation energy means the reaction occurs much faster. Oxygen gas is produced at a rapid rate, causing the detergent to foam up.
The catalase itself isn't used up in the reaction. A chemical which lowers the activation energy for a chemical reaction, but doesn't react itself, is called a catalyst.
Applications
Catalysts have many roles in industry. Many beneficial chemical reactions have high activation energies, meaning they normally take a long time, or require high temperatures to take place. Catalysts are used to make reactions occur more readily, making it cheaper to produce the end product.
As the catalyst doesn't react itself only a relatively small amount of catalyst is needed for large-scale industrial reactions.
By Patrick Mahony
More information
View the online version
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