1. Video Tutorial on Kinetics and methodsused to measure rate of chemical reactionsfor IA experiments. Prepared by Lawrence Kok http://lawrencekok.blogspot.com

2. Techniques Used to measure Rate of Reactions Reaction between CaCO3 with HCI can be measured using THREE different methods CaCO3 + 2HCI CaCI2 + CO2 + H2OMethod 1Method 2Method 3Method 1 Rate of reaction measured as in mass CaCO3 over time Apparatus is set up shown below where initial mass and its contents are recordedProcedureCaCO3 + 2HCI CaCI2 + CO2 + H2O (CaCO3 is limiting, HCI is excess)Pour 50ml of 0.5M HCI into conical flask and place it on electronic balanceWeigh accurately 1.00g of CaCO3 and place it on electronic balance Record down the total mass and add CaCO3 into flask and start stopwatch immediately Mass of flask is recorded for every 1 min interval shown in table 3. Techniques Used to measure Rate of Reactions Reaction between CaCO3 with HCI can be measured using THREE different methodsCaCO3 + 2HCI CaCI2 + CO2 + H2O Method 1 Method 2 Method 3Method 1Results Repeat expt using 1.0M HCI Rate of reaction using 1.0M HCI is faster > than 0.5M HCI Research Questions possible Effect of Temperature, Surface area of CaCO3, Concentration on rate of reaction 4. Techniques Used to measure Rate of Reactions Reaction between CaCO3 with HCI can be measured using THREE different methodsCaCO3 + 2HCI CaCI2 + CO2 + H2O Method 1 Method 2Method 3Method 2 Rate of reaction measured as in volume CO2 over time Apparatus is set up with burette filled with water and initial volume recordedProcedure CaCO3 + 2HCI CaCI2 + CO2 + H2O (CaCO3 is limiting, HCI is excess) Excess CaCO3 added to 20ml of 0.5M HCI and CO2 released is recorded at 1 min interval 5. Techniques Used to measure Rate of Reactions Reaction between CaCO3 with HCI can be measured using THREE different methodsCaCO3 + 2HCI CaCI2 + CO2 + H2O Method 1 Method 2 Method 3Method 2Results Repeat expt using 1.0M HCI Rate of reaction using 1.0M HCI is faster > than 0.5M HCI Research Questions possible Effect of Temperature, Surface area of CaCO3, Concentration on rate of reaction 6. Techniques Used to measure Rate of Reactions Reaction between CaCO3 with HCI can be measured using THREE different methodsCaCO3 + 2HCI CaCI2 + CO2 + H2O Method 1 Method 2 Method 3Method 3 Rate of reaction measured as in pressure CO2 over time Apparatus is set up where the test tube is link to gas pressure sensorProcedure CaCO3 + 2HCI CaCI2 + CO2 + H2O (CaCO3 is limiting, HCI is excess) Excess CaCO3 added to 10ml of 0.5M HCI and pressure due to CO2 released is recordedat 1 min interval 7. Techniques Used to measure Rate of Reactions Reaction between CaCO3 with HCI can be measured using THREE different methodsCaCO3 + 2HCI CaCI2 + CO2 + H2O Method 1 Method 2 Method 3Method 3Results Repeat expt using 1.0M HCI Rate of reaction using 1.0M HCI is faster > than 0.5M HCI Research Questions possible Effect of Temperature, Surface area of CaCO3, Concentration on rate of reaction 8. Techniques Used to measure Rate of Reactions Reaction between Na2S2O3 with HCI can be measured using TWO different methodsNa2S2O3 + 2HCI 2NaCI2 + SO2 + H2O + S Method 1 Method 2Method 1 Rate of reaction measured as in mass sulphur or 1/ Time for Disappearance of cross X Apparatus is set up shown belowProcedure Na2S2O3 + 2HCI 2NaCI2 + SO2 + H2O + S (Na2S2O3 is limiting, HCI is excess)Pour 50ml of 0.2M HCI into conical flask and place it on top of white paper with cross X Pour 5.0ml of 0.1M HCI into flask X is view vertically from the top and record the time for X to disappear Repeat expt with different Na2S2O3 concentration 9. Techniques Used to measure Rate of Reactions Reaction between Na2S2O3 with HCI can be measured using TWO different methodsNa2S2O3 + 2HCI 2NaCI2 + SO2 + H2O + SMethod 1 Method 2Method 1Results As concentration increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order of reaction with respect to HCI and Na2S2O3 concentration ? 10. Techniques Used to measure Rate of Reactions Reaction between Na2S2O3 with HCI can be measured using TWO different methodsNa2S2O3 + 2HCI 2NaCI2 + SO2 + H2O + S Method 1 Method 2 Method 2 Rate of reaction measure as light intensity or 1/Time for light intensity to drop due to sulphur formation Apparatus is set up shown belowProcedure Na2S2O3 + 2HCI 2NaCI2 + SO2 + H2O + S (Na2S2O3 is limiting, HCI is excess) Pipette 1ml 0.2M S2O3 of into cuvette Place it above a light sensor and measure the light intensity Pipette 0.1ml of 1.0M HCI into cuvette and start data collection. Record the initial time Record the time for light intensity to drop (due to sulphur formation) Repeat expt with different Na2S2O3 concentration 11. Techniques Used to measure Rate of Reactions Reaction between Na2S2O3 with HCI can be measured using TWO different methods Na2S2O3 + 2HCI 2NaCI2 + SO2 + H2O + SMethod 1 Method 2Method 2Results As concentration increases , rate increases Effect of Temperature and Concentration on the rate of reactionResearch Questions possible What is the order with respect to HCI and Na2S2O3 concentration ? 12. Techniques Used to measure Rate of Reactions H2O2- Oxidising Agent Iodine Clock Reaction H2O2 + 2I +- 2H+ 2H2O + I2I- - Reducing Agent I2 + 2S203 S406 2- + 2I - 2-S2032- - Reduces I2 to I I2 - Once all used up, I2 will react I2 + starch Blue black with starch forming blue blackReaction between H2O2 with I - can be measured using TWO different methodsMethod 1Method 2Method 1 Rate of reaction measure as in mass I2 or 1/Time for disappearance of X due to blue black formation Apparatus is set up shown belowProcedure H2O2 + 2KI + 2HCI 2KCI + 2H2O + I2 (KI is limiting, H2O2 is excess) Pipette 5ml 3% H2O2, 5ml of 0.1M HCI, 1ml 1% starch, 1ml of 0.001M S2O3 of into conical flask Place it on top of white paper with cross X and pipette 5 ml of 0.1M KI into flask X is view vertically from the top and record the time for X to disappear Repeat expt with different KI concentration 13. Techniques Used to measure Rate of Reactions H2O2- Oxidising Agent Iodine Clock Reaction H2O2 + 2I + - 2H+ 2H2O + I2I- - Reducing Agent I2 + 2S203 S406 2- + 2I -2- S2032- - Reduces I2 to I I2 - Once all used up, I2 will react I2 + starch Blue black with starch forming blue blackReaction between H2O2 with I - can be measured using TWO different methodsMethod 1Method 2Method 1Results As concentration increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order or reaction with respect to H2O2 and KI concentration ? 14. Techniques Used to measure Rate of Reactions H2O2- Oxidising Agent Iodine Clock Reaction H2O2 + 2I +- 2H+ 2H2O + I2I- - Reducing Agent I2 + 2S203 S406 2- + 2I - 2-S2032- - Reduces I2 to I I2 - Once all used up, I2 will react I2 + starch Blue black with starch forming blue blackReaction between H2O2 with I - can be measured using TWO different methodsMethod 1Method 2Method 2 Rate of reaction measure as in absorbance or 1/Time for absorbance to increase (blue black formation) Apparatus is set up shown belowProcedure H2O2 + 2KI + 2HCI 2KCI + 2H2O + I2 (KI is limiting, H2O2 is excess) Pipette 0.5ml 3% H2O2, 0.5ml of 0.1M HCI, 0.1ml 1% starch, 0.1ml of 0.001M S2O3 of into cuvette Pipette 0.5ml of 0.1M KI in cuvette and record the initial time Record the time for when absorbance rises (formation of blue black colouration) Repeat expt using 0.5ml of different KI concentration 15. Techniques Used to measure Rate of Reactions H2O2- Oxidising Agent Iodine Clock Reaction H2O2 + 2I +- 2H2O + I22H+I- - Reducing Agent I2 + 2S203 S406 2- + 2I - 2-S2032- - Reduces I2 to I I2 - Once all used up, I2 will react I2 + starch Blue black with starch forming blue blackReaction between H2O2 with I - can be measured using TWO different methods Method 1 Method 2Method 2Results As concentration increases , rate increases Effect of Temperature and Concentration on the rate of reactionResearch Questions possible What is the order of reaction with respect to H2O2 and KI concentration ? 16. Techniques Used to measure Rate of ReactionsS2O82- - Oxidising Agent Iodine Clock ReactionS2O82- + 2I 2SO4 + I2-2- I- - Reducing AgentI2 + 2S2032- S406 2- + 2I - S2032- - Reduces I2 to I I2- Once all used up, I2 will reactI2 + starch Blue blackwith starch forming blue blackReaction between S2O82- with I - can be measured using TWO different methods Method 1Method 2Method 1 Rate of reaction measure as in mass I2 or 1/Time for disappearance of X due to blue black formation Apparatus is set up shown belowProcedure S2O82- + 2I - 2SO42- + I2 (KI is limiting, S2O82- is excess) Pipette 5ml 0.1M KI, 5ml of 0.001M S2O3 ,1ml 1% starch into conical flask Place it on top of white paper with cross X and pipette 5 ml of 0.1M S2O82- into flask X is view vertically from the top and record the time for X to disappear Repeat expt with different KI concentration 17. Techniques Used to measure Rate of ReactionsS2O82- - Oxidising Agent Iodine Clock Reaction S2O82- + 2I 2SO4 + I2 -2-I- - Reducing Agent I2 + 2S2032- S406 2- + 2I -S2032- - Reduces I2 to I I2- Once all used up, I2 will react I2 + starch Blue black with starch forming blue blackReaction between S2O82- with I - can be measured using TWO different methods Method 1Method 2Method 1Results As concentration increases , rate increases Effect of Temperature and Concentration on the rate of reactionResearch Questions possible What is the order of reaction with respect to S2O82- and KI concentration ? 18. Techniques Used to measure Rate of ReactionsS2O82- - Oxidising Agent Iodine Clock ReactionS2O82- + 2I 2SO4 + I2-2- I- - Reducing AgentI2 + 2S2032- S406 2- + 2I - S2032- - Reduces I2 to I I2- Once all used up, I2 will reactI2 + starch Blue blackwith starch forming blue blackReaction between S2O82- with I - can be measured using TWO different methods Method 1 Method 2Method 2 Rate of reaction measure as in absorbance or 1/Time for absorbance to increase (blue black formation) Apparatus is set up shown belowProcedure S2O82- + 2I - 2SO42- + I2 (KI is limiting, S2O82- is excess) Pipette 0.5ml 0.1M KI, 0.1ml of 0.001M S2O3 , 0.5ml 1% starch into cuvette Place cuvette into a visible spectrophotometer and start data collection Pipette 0.5ml of 0.1M S2O82- into cuvette and record the initial time Record the time for when absorbance rises (formation of blue black colouration) Repeat expt using 0.5ml of different KI concentration 19. Techniques Used to measure Rate of ReactionsS2O82- - Oxidising Agent Iodine Clock Reaction S2O82- + 2I 2SO4 + I2 -2-I- - Reducing Agent I2 + 2S2032- S406 2- + 2I -S2032- - Reduces I2 to I I2- Once all used up, I2 will react I2 + starch Blue black with starch forming blue blackReaction between S2O82- with I - can be measured using TWO different methods Method 1Method 2Method 2Results As concentration increases , rate increases Effect of Temperature and Concentration on the rate of reactionResearch Questions possible What is the order of reaction with respect to S2O82- and KI concentration ? 20. Techniques Used to measure Rate of Reactions Reaction between H2O2 with KI can be measured using TWO different methods 2H2O2 O2 + 2H2O (KI as catalyst)Method 1Method 2Method 1 Rate of reaction measured as in volume O2 over time Apparatus is set up with burette filled with water and initial volume recordedProcedure 2H2O2 O2 + 2H2O (H2O2 is limiting, KI is excess) Pipette 1ml of 1.0M KI to 20ml of 1.5% H2O2 and O2 released is recorded at 1 min interval Expt repeated using 3% H2O2 concentration 21. Techniques Used to measure Rate of Reactions Reaction between H2O2 with KI can be measured using TWO different methods2H2O2 O2 + 2H2O (KI as catalyst) Method 1 Method 2 Method 1Results As concentration increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order of reaction with respect to H2O2 concentration ? Effect of different catalyst on the rate of reaction. 22. Techniques Used to measure Rate of Reactions Reaction between H2O2 with KI can be measured using TWO different methods 2H2O2 O2 + 2H2O (KI as catalyst)Method 1 Method 2Method 2 Rate of reaction measured as in pressure of O2 over time Apparatus is set up with flask link to gas pressure sensorProcedure 2H2O2 O2 + 2H2O (H2O2 is limiting, KI is excess) Pipette 1ml of 1.0M KI to 20ml of 1.5% H2O2 and O2 released is recorded at 1 min interval Expt repeated using 3% H2O2 concentration 23. Techniques Used to measure Rate of Reactions Reaction between H2O2 with KI can be measured using TWO different methods2H2O2 O2 + 2H2O (KI as catalyst) Method 1 Method 2 Method 2Results As concentration increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order of reaction with respect to H2O2 concentration ? Effect of different catalyst on the rate of reaction. 24. Techniques Used to measure Rate of Reactions2Fe3+ + 2I - 2Fe2+ + I2Fe 3+ - Oxidising Agent I-- Reducing AgentReaction between Fe3+ + I - can be measured using TWO different methods Method 1Method 2Method 1 Rate of reaction measure as in absorbance or Increase in absorbance due to iodine Apparatus is set up shown belowProcedure 2Fe3+ + 2I - 2Fe2+ + I2 (I - is limiting, Fe3+ is excess) Pipette 1.5ml 0.02M Fe3+into cuvette. Determine the max for Fe3+ solution (450nm) Set spectrophotometer to Absorbance vs time mode and select = 450nm Pipette 1.0ml of 0.02M Fe3+, 1.0ml of KI into cuvette and mix them Place cuvette into spectrophotometer and measure the absorbance increase due to I2 formation Repeat expt using 1.0ml of different KI concentration 25. Techniques Used to measure Rate of Reactions2Fe3+ + 2I - 2Fe2+ + I2Fe 3+ - Oxidising Agent I-- Reducing AgentReaction between Fe3+ + I - can be measured using TWO different methods Method 1Method 2Method 1Results As concentration increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order of reaction with respect to Fe3+ and I - concentration ? 26. Techniques Used to measure Rate of Reactions Fe 3+ - Oxidising Agent 2Fe 3++ 2I - 2Fe 2++ I2 I-- Reducing AgentReaction between Fe3+ + I - can be measured using TWO different methodsMethod 1 Method 2Method 2 Rate of reaction measure as in concentration of I2 or Increase in I2 concentration over time Apparatus is set up shown belowProcedure 2Fe3+ + 2I - 2Fe2+ + I2 (I - is limiting, Fe3+ is excess) Pipette 25ml of 0.02M KI , 25ml of 0.02M Fe3+ into a conical flask. Start the time For every 5mins, pipette 10ml of solution mixture into a flask and titrate with S2O32-(Reaction mixture contains I2 formed which will react with S2O32-) Amt of I2 produced can be determine. I2 + 2S2032- S4062- + 2I ( Mole ratio is 1:2) Perform titration until volume of S2O32- added remains constant (Conc I2 produced remains constant) 27. Techniques Used to measure Rate of ReactionsFe 3+ - Oxidising Agent2Fe 3+ + 2I - 2Fe 2+ + I2 I-- Reducing AgentReaction between Fe3+ + I - can be measured using TWO different methods Method 1 Method 2Method 2ResultsCalculations At time 5mins Vol of S2032- is 6.0ml Amt of S2032- = M x V = 0.2 x 0.006 = 0.0012molFor a reaction : 2Fe3+ + 2I - 2Fe2+ + I2 Concentration of product I2 increases with time Rate of reaction decreases with time, as the gradient is less steep with time As concentration of reactants decreases, rate of I2 production decreases 28. Techniques Used to measure Rate of Reactions Reaction between I2 + CH3COCH3 can be measured using TWO different methodsI2 + CH3COCH3 CH3COCH2I + H+ + I - Method 1 Method 2Method 1 Rate of reaction measure as in absorbance or Decrease in absorbance due to iodine Apparatus is set up shown belowProcedure I2 + CH3COCH3 CH3COCH2I + H+ + I - (CH3COCH3 is limiting, I2 is excess) Rate is monitored by disappearance of I2 yellowish solution over time Pipette 2ml of 0.002M I2 into cuvette. Find the max for I2 ( max = 520nm) Set colorimeter to Absorbance vs Time mode Pipette 0.4ml of I2 solution, 0.4ml of 2M HCI and 1ml water into a cuvette Start data collection at max = 520nm Pipette 0.4ml of 0.2M CH3COCH3 into cuvette and record the drop in absorbance over time Repeat expt using of different CH3COCH3 concentration . 29. Techniques Used to measure Rate of ReactionsReaction between I2 + CH3COCH3 can be measured using TWO different methods I2 + CH3COCH3 CH3COCH2I + H+ + I -Method 1Method 2Method 1Results As concentration CH3COCH3 increases , decrease in absorbance over time increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order of reaction with respect to H+, CH3COCH3 and I2 concentration ? 30. Techniques Used to measure Rate of Reactions Reaction between I2 + CH3COCH3 can be measured using TWO different methodsI2 + CH3COCH3 CH3COCH2I + H+ + I - Method 1 Method 2Method 2 Rate of reaction measure as in absorbance or Decrease in concentration of iodineProcedure I2 + CH3COCH3 CH3COCH2I + H+ + I - (CH3COCH3 is limiting, I2 is excess) Rate is monitored by disappearance of I2 yellowish solution over time Pipette 2ml of 0.002M I2 into cuvette. Find the max for I2 ( max = 520nm) Set colorimeter to Absorbance vs Concentration mode. (Standard calibration curve) Prepare a standard calibration curve for Absorbance vs I2 concentration shown belowPipette 0.4ml of I2, 0.4ml of 2M HCI and 1ml water into a cuvette. Start data collection at max = 520nmPipette 0.4ml of 0.2M CH3COCH3 into cuvette and record the drop in absorbance over time Repeat expt using of different CH3COCH3 concentration . 31. Techniques Used to measure Rate of ReactionsReaction between I2 + CH3COCH3 can be measured using TWO different methods I2 + CH3COCH3 CH3COCH2I + H+ + I -Method 1Method 2Method 2ResultsConvert Absorbance I2 to Concentration I2using standard calibration curve As concentration CH3COCH3 increases , decrease in absorbance over time increases , rate increases Research Questions possible Effect of Temperature and Concentration on the rate of reaction What is the order of reaction with respect to H+, CH3COCH3 and I2 concentration ? 32. AcknowledgementsThanks to source of pictures and video used in this presentationThanks to Creative Commons for excellent contribution on licenseshttp://creativecommons.org/licenses/Prepared by Lawrence KokCheck out more video tutorials from my site and hope you enjoy this tutorialhttp://lawrencekok.blogspot.com