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Chemistry
Setup:
In this procedure the amount of Acid was kept constant at 1 ml. You can increase/decrease the amount of acid depending on time.
The concentration of Sodium Thiosulphate was altered by adding varying amounts of distilled water.
Sodium Thiosulphate (ml)
3
2.5
2.0
1.5
1.0
Distilled water (ml)
0
0.5
1.0
1.5
2.0
Hydrochloric Acid (ml)
1
1
1
1
1
------------------------------------------------------------------------------------
Total volume of liquid (ml)
4
4
4
4
4
For this experiment, you need to make a tube of cardboard to channel the light to the SmartEye sensor. In this example, we cut the
profi le of the test tube into one end of the tube so that the light has to pass through the test tube.
Method:
1. Connect Voyager to the computer.
2. Set up the datalogging facility of the software. (For LogIT Lab use ‘Autolog’ otherwise set the time span between 5 and 15 minutes.)
3. Carefully measure out 3 ml of Sodium Thiosulphate and place it into the test-tube.
4. Start logging.
5. After about 15 seconds, add 1 ml of Hydrochloric Acid. (The dropping of the acid should be enough to mix the reactants.)
6. Keep collecting data until the light levels no longer drop ie. the reaction has fi nished.
7. Stop logging and then repeat for the different concentrations by adding distilled water shown in the above table.
Note: It is important to clean the test-tube thoroughly with distilled water between readings.
The reaction time can be obtained from the graph from where the plot starts to fall to where the plot levels off again. The rate of the
reaction can be determined by calculating how much sulphur was produced in the recorded time.
Since we can assume that the amount of sulphur obtained is the same, the rate of reaction can be
expressed as:- Rate of reaction = 1 / Time taken
Results:
What do the results show about how the rate of reaction can be changed?
How does this method ensure it was a fair test?
Why was it important to ensure the test-tube was thoroughly cleaned each time?
Going further:
How might the temperature affect the reaction rate?
How might this experiment relate to reactions at home?