The Kinetocs Experiment of Iodide Ions and Persulphate Ions.
The catalytic effect of D-block ions and the kinetics of reactions iodine clock reaction:
By Stephen Parsons 6K2
Centre number: 61813
Candidate number: 8270
Table of Contents My aim and my reaction: 3 Rate of reaction: 4 Activation enthalpy: 5 Collision theory: 6 The effect of temperature on reaction rate: 7 The effect of concentration on reaction rate: 7 The effect of a catalyst on reaction rate: 8 D-block elements: 9 The effect of extra kinetic energy (from stirring etc.): 10 Where do we use D-block ion catalysts? 10 Arrhenius equation: 12 Orders of reaction: 10 Oxidation states of D-block ions: 13 Electronic configuration and transition metals: 13 Experiment: 13 Method: 14 Risk assessment: 15 How to make my standard solutions of each of my reactants: 15 Changing the concentration of potassium iodide: 18 Changing the concentration of potassium peroxodisulphate: 19 Changing the quantity of iron (III) sulphate: 20 Changing the temperature at which different runs are done at: 21 Changing the temperature of the reaction and using a catalyst: 21 Results: 22 Iron (III) sulphate: 22 Potassium iodide: 27 Potassium peroxodisulphate: 31 Temperature change: 35 Arrhenius equation: 37 Percentage error: 42 Conclusion: 43 Evaluation: 44 Bibliography 46
Introduction:
My aim and my reaction:
I will be adding Potassium iodide, distilled water, Potassium peroxodisulphate (VI), Sodium thiosulphate (VI), starch and when varying the use of a catalyst I will also add Iron (III) sulphate. I will start a stop watch when I mix the appropriate concentrations of solutions together, When I react these solutions a slow reaction will occur, tri-iodide is formed and this then reacts with the sodium thiosulphate(VI) this will happen until all of the sodium thiosulphate has reacted with the tri-iodide that is produced. The further tri-iodide that is produced is reacts with the starch in the solution and this changes the solutions colour to a bluey-black and
By Stephen Parsons 6K2
Centre number: 61813
Candidate number: 8270
Table of Contents My aim and my reaction: 3 Rate of reaction: 4 Activation enthalpy: 5 Collision theory: 6 The effect of temperature on reaction rate: 7 The effect of concentration on reaction rate: 7 The effect of a catalyst on reaction rate: 8 D-block elements: 9 The effect of extra kinetic energy (from stirring etc.): 10 Where do we use D-block ion catalysts? 10 Arrhenius equation: 12 Orders of reaction: 10 Oxidation states of D-block ions: 13 Electronic configuration and transition metals: 13 Experiment: 13 Method: 14 Risk assessment: 15 How to make my standard solutions of each of my reactants: 15 Changing the concentration of potassium iodide: 18 Changing the concentration of potassium peroxodisulphate: 19 Changing the quantity of iron (III) sulphate: 20 Changing the temperature at which different runs are done at: 21 Changing the temperature of the reaction and using a catalyst: 21 Results: 22 Iron (III) sulphate: 22 Potassium iodide: 27 Potassium peroxodisulphate: 31 Temperature change: 35 Arrhenius equation: 37 Percentage error: 42 Conclusion: 43 Evaluation: 44 Bibliography 46
Introduction:
My aim and my reaction:
I will be adding Potassium iodide, distilled water, Potassium peroxodisulphate (VI), Sodium thiosulphate (VI), starch and when varying the use of a catalyst I will also add Iron (III) sulphate. I will start a stop watch when I mix the appropriate concentrations of solutions together, When I react these solutions a slow reaction will occur, tri-iodide is formed and this then reacts with the sodium thiosulphate(VI) this will happen until all of the sodium thiosulphate has reacted with the tri-iodide that is produced. The further tri-iodide that is produced is reacts with the starch in the solution and this changes the solutions colour to a bluey-black and
Bibliography: 1. http://www.avogadro.co.uk/definitions/hactivation.htm. http://www.avogadro.co.uk/definitions/hactivation.htm. [Online] 11 31, 2011. [Cited: 11 31, 2011.] http://www.avogadro.co.uk/definitions/hactivation.htm. 2. http://www.chemguide.co.uk/physical/basicrates/temperature.html. http://www.chemguide.co.uk/physical/basicrates/temperature.html. [Online] september 11, 2011. [Cited: september 11, 2011.] http://www.chemguide.co.uk/physical/basicrates/temperature.html. 3. http://www.physchem.co.za/OB12-che/catalysis.htm. http://www.physchem.co.za/OB12-che/catalysis.htm. [Online] september 11, 2011. [Cited: september 11, 2011.] http://www.physchem.co.za/OB12-che/catalysis.htm. 4. http://www.docbrown.info/page03/ASA2rates.htm. http://www.docbrown.info/page03/ASA2rates.htm. [Online] http://www.docbrown.info/page03/ASA2rates.htm, september 4, 2011. [Cited: september 4, 2011.] http://www.docbrown.info/page03/ASA2rates.htm. 5. http://www.chemguide.co.uk/inorganic/transition/features.html. http://www.chemguide.co.uk/inorganic/transition/features.html. [Online] september 2, 2011. [Cited: september 2, 2011.] http://www.chemguide.co.uk/inorganic/transition/features.html. 6. http://www.chemguide.co.uk/physical/basicrates/arrhenius.html. http://www.chemguide.co.uk/physical/basicrates/arrhenius.html. [Online] 11 31, 2011. [Cited: 11 31, 2011.] http://www.chemguide.co.uk/physical/basicrates/arrhenius.html. 11. chemical ideas chapter 10. [book auth.] ocr. chemical ideas. s.l. : heinemann, 2011. 12