RP7-a-Measuring the initial rate of a reaction by an initial rate method Flashcards
1
Q
Iodine Clock Required practical 7a
A
2
Q
Describe what happens in this reaction?
A
Hydrogen peroxide reacts with iodide ions to form iodine and the thiosulfate ion immediately reacts with iodine:
H2O2(aq) + 2H+(aq) + 2I-(aq) → I2(aq) +2H2O(l)
2S2O32-(aq) + I2(aq) → 2I-(aq) + S4O62-(aq)
3
Q
Describe how this practical would be carried out?
A
- Fill the 50 cm3 burette with potassium iodide solution.
2.Transfer 10.0 cm3 of hydrogen peroxide solution from a burette to a 100 cm3 beaker
3.Use a 50 cm3 measuring cylinder to add 25 cm3 of sulfuric acid to a 250 cm3
beaker.
4.Use a 25 cm3 measuring cylinder to add 20 cm3 of distilled (deionised) water into the 250 cm3 beaker.
5.Use a plastic dropping pipette to add about 1 cm3 of starch solution to this beaker. - Use the burette to add 5.0 cm3 of potassium iodide solution to the mixture in the 250 cm3 beaker.
- Finally, add 5.0 cm3 of sodium thiosulfate solution from a burette to the mixture in the 250 cm3 beaker.
- Stir the mixture in the 250 cm3 beaker. Pour the hydrogen peroxide solution from the 100 cm3 beaker into the 250 cm3 beaker and immediately start the timer.
- Stop the timer when the mixture in the 250 cm3 beaker turns blue-black. Record the time.
- Repeat steps in four further experiments changing the concentration of
potassium iodide. - Plot a graph of initial rate (y) versus concentration (x) to determine the order.
4
Q
how can we improve accuracy of this reaction?
A
use a colorimeter to minimise human errors
5
Q
From these results what must need to be calculated in order to determine the order?
A
- calculate the moles of potassium iodine in each reaction
- Then calculate the final concentration of potassium iodide in the solution (Concentration = Moles/ total volume of all reactants)
- Then we can calculate the rate of reaction by Rate = 1/t
- We can then plot our results on a graph and determine the order
6
Q
Finished.
A