- Put a certain mass of a metal, let's say magnesium, into a beaker with x amount of sulphuric acid in it (let's say 100ml). Do this with a block of it.
- Time the reaction, record results
- Repeat step 1 but use another form (i.e. powder)
- Time the reaction again, record results
- Keep repeating with different forms (i.e. strips, etc.), making sure to always use the same mass of the same metal with the same amount of sulphuric acid.
- You should see that the powder will have the quickest reaction because it has the largest surface area.
Concentration
- Put a conical flask on a mini whiteboard on a table. Draw an x in the middle of the whiteboard. Place the conical flask on top
- Presume that 0.2g of sulphur is produced
- Keep changing the ratio of sodium thiosulfate and water, always adding the same amount of hydrochloric acid and measure how long it takes for the cross to be obscured
- Repeat as required
- From this, calculate the concentration (moles ÷ volume = concentration)
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| Figure 1: My sad looking drawing of the experiment, but I hope you can tell what I mean |
Temperature
- Put x amount of magnesium into y amount of sulphuric acid at room temperature
- Time reaction, record results
- Repeat at different temperatures
- You will see that the greater the temp, the faster the rate of reaction
Use of a catalyst
- Put x amount of hydrogen peroxide into a conical flask with y amount of manganese dioxide
- Time how long it takes for the oxygen to displace all the water in the gas jar
- Repeat, increasing the amount of manganese dioxide each time. Yes, you still have to time the reaction. Keep amount x (of hydrogen peroxide) the same
- You will see that the more catalyst you have, the faster the rate of reaction
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| Figure 2: My second sad looking diagram...I hope you still have some idea of what I mean... |
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