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Techniques Used to measure Rate of Reactions
Reaction between CaCO3 with HCI can be measured using THREE different methods
CaCO3 + 2HCI → CaCI2 + CO2 + H2O
Method 1 Method 2 Method 3
Method 1
• Rate of reaction measured as Δ in mass CaCO3 over time
• Apparatus is set up shown below where initial mass and its contents are recorded
Procedure
•CaCO3 + 2HCI → CaCI2 + CO2 + H2O (CaCO3 is limiting, HCI is excess)
•Pour 50ml of 0.5M HCI into conical flask and place it on electronic balance
•Weigh 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
• Repeat expt using 1.0M HCI
• Rate of reaction using 1.0M HCI is faster > than 0.5M HCI
Results
Research Questions possible
• Effect of Temperature, Surface area of CaCO3, Concentration on rate of reaction
Techniques Used to measure Rate of Reactions
Reaction between CaCO3 with HCI can be measured using THREE different methods
CaCO3 + 2HCI → CaCI2 + CO2 + H2O
Method 1 Method 2 Method 3
Method 1
Techniques Used to measure Rate of Reactions
Reaction between CaCO3 with HCI can be measured using THREE different methods
CaCO3 + 2HCI → CaCI2 + CO2 + H2O
Method 1 Method 2 Method 3
Method 2
• Rate of reaction measured as Δ in volume CO2 over time
• Apparatus is set up with burette filled with water and initial volume recorded
Procedure
• 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
• Repeat expt using 1.0M HCI
• Rate of reaction using 1.0M HCI is faster > than 0.5M HCI
Results
Research Questions possible
• Effect of Temperature, Surface area of CaCO3, Concentration on rate of reaction
Techniques Used to measure Rate of Reactions
Reaction between CaCO3 with HCI can be measured using THREE different methods
CaCO3 + 2HCI → CaCI2 + CO2 + H2O
Method 1 Method 2 Method 3
Method 2
Techniques Used to measure Rate of Reactions
Reaction between CaCO3 with HCI can be measured using THREE different methods
CaCO3 + 2HCI → CaCI2 + CO2 + H2O
Method 1 Method 2 Method 3
Method 3
• Rate of reaction measured as Δ in pressure CO2 over time
• Apparatus is set up where the test tube is link to gas pressure sensor
Procedure
• 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 recorded
at 1 min interval
• Repeat expt using 1.0M HCI
• Rate of reaction using 1.0M HCI is faster > than 0.5M HCI
Results
Research Questions possible
• Effect of Temperature, Surface area of CaCO3, Concentration on rate of reaction
Techniques Used to measure Rate of Reactions
Reaction between CaCO3 with HCI can be measured using THREE different methods
CaCO3 + 2HCI → CaCI2 + CO2 + H2O
Method 1 Method 2 Method 3
Method 3
Techniques Used to measure Rate of Reactions
Reaction between Na2S2O3 with HCI can be measured using TWO different methods
Na2S2O3 + 2HCI → 2NaCI2 + SO2 + H2O + S
Method 1 Method 2
Method 1
• Rate of reaction measured as Δ in mass sulphur or 1/ Time for Disappearance of cross X
• Apparatus is set up shown below
Procedure
• 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
Techniques Used to measure Rate of Reactions
Reaction between Na2S2O3 with HCI can be measured using TWO different methods
Na2S2O3 + 2HCI → 2NaCI2 + SO2 + H2O + S
Method 1 Method 2
Method 1
• As concentration increases ↑ , rate increases ↑
Results
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 ?
Techniques Used to measure Rate of Reactions
Reaction between Na2S2O3 with HCI can be measured using TWO different methods
Na2S2O3 + 2HCI → 2NaCI2 + SO2 + H2O + S
Method 1 Method 2
Method 2
• Rate of reaction measure as Δ light intensity or 1/Time for light intensity to drop due to sulphur formation
• Apparatus is set up shown below
Procedure
• 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
Techniques Used to measure Rate of Reactions
Reaction between Na2S2O3 with HCI can be measured using TWO different methods
Na2S2O3 + 2HCI → 2NaCI2 + SO2 + H2O + S
Method 1 Method 2
Method 2
• As concentration increases ↑ , rate increases ↑
Results
Research Questions possible • Effect of Temperature and Concentration on the rate of reaction
• What is the order with respect to HCI and Na2S2O3 concentration ?
Techniques Used to measure Rate of Reactions
Reaction between H2O2 with I - can be measured using TWO different methods
H2O2 + 2I - + 2H+ → 2H2O + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
H2O2 - Oxidising Agent I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Method 1
• Rate of reaction measure as Δ in mass I2 or 1/Time for disappearance of X due to blue black formation
• Apparatus is set up shown below
• 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
Procedure
Techniques Used to measure Rate of Reactions
Reaction between H2O2 with I - can be measured using TWO different methods
H2O2 + 2I - + 2H+ → 2H2O + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
H2O2 - Oxidising Agent I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Method 1
Results
• 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 ?
Techniques Used to measure Rate of Reactions
Reaction between H2O2 with I - can be measured using TWO different methods
H2O2 + 2I - + 2H+ → 2H2O + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
H2O2 - Oxidising Agent I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Method 2
• Rate of reaction measure as Δ in absorbance or 1/Time for absorbance to increase (blue black formation)
• Apparatus is set up shown below
• 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
Procedure
Techniques Used to measure Rate of Reactions
Reaction between H2O2 with I - can be measured using TWO different methods
H2O2 + 2I - + 2H+ → 2H2O + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
H2O2 - Oxidising Agent I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Results
Research Questions possible • Effect of Temperature and Concentration on the rate of reaction
• What is the order of reaction with respect to H2O2 and KI concentration ?
• As concentration increases ↑ , rate increases ↑
Method 2
Techniques Used to measure Rate of Reactions
Reaction between S2O82- with I - can be measured using TWO different methods
S2O82- + 2I - → 2SO4
2- + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
S2O82- - Oxidising Agent
I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Method 1
Procedure
• Rate of reaction measure as Δ in mass I2 or 1/Time for disappearance of X due to blue black formation
• Apparatus is set up shown below
• S2O82- + 2I - → 2SO4
2- + 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
Techniques Used to measure Rate of Reactions
Reaction between S2O82- with I - can be measured using TWO different methods
S2O82- + 2I - → 2SO4
2- + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
S2O82- - Oxidising Agent
I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Method 1
Results
Research Questions possible
• As concentration increases ↑ , rate increases ↑
• Effect of Temperature and Concentration on the rate of reaction
• What is the order of reaction with respect to S2O82- and KI concentration ?
Techniques Used to measure Rate of Reactions
Reaction between S2O82- with I - can be measured using TWO different methods
S2O82- + 2I - → 2SO4
2- + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
S2O82- - Oxidising Agent
I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Method 2
Procedure
• Rate of reaction measure as Δ in absorbance or 1/Time for absorbance to increase (blue black formation)
• Apparatus is set up shown below
• S2O82- + 2I - → 2SO4
2- + 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
Techniques Used to measure Rate of Reactions
Reaction between S2O82- with I - can be measured using TWO different methods
S2O82- + 2I - → 2SO4
2- + I2
I2 + 2S2032- → S406 2- + 2I -
I2 + starch → Blue black
S2O82- - Oxidising Agent
I - - Reducing Agent S203
2- - Reduces I2 to I –
I2 - Once all used up, I2 will react with starch forming blue black
Iodine Clock Reaction
Method 1 Method 2
Results
Research Questions possible
• As concentration increases ↑ , rate increases ↑
• Effect of Temperature and Concentration on the rate of reaction
• What is the order of reaction with respect to S2O82- and KI concentration ?
Method 2
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 2
Method 1
• Rate of reaction measured as Δ in volume O2 over time
• Apparatus is set up with burette filled with water and initial volume recorded
Procedure
• 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
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 2
Method 1
Results
Research Questions possible
• As concentration increases ↑ , rate increases ↑
• 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.
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 2
Method 2
• Rate of reaction measured as Δ in pressure of O2 over time
• Apparatus is set up with flask link to gas pressure sensor
Procedure
• 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
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 2
Method 2
Results
Research Questions possible
• As concentration increases ↑ , rate increases ↑
• 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.
Techniques Used to measure Rate of Reactions
Reaction between Fe3+ + I - can be measured using TWO different methods
Fe 3+ - Oxidising Agent I - - Reducing Agent
Method 1 Method 2
Method 1
• Rate of reaction measure as Δ in absorbance or Increase in absorbance due to iodine
• Apparatus is set up shown below
• 2Fe3+ + 2I - → 2Fe2+ + I2 (I -
is limiting, Fe3+ is excess)
• Pipette 1.5ml 0.02M Fe3+into cuvette. Determine the λ max for Fe3+ solution (450nm)
• Set spectrophotometer to Absorbance vs time mode and select λ = 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
Procedure
2Fe3+ + 2I - → 2Fe2+ + I2
Techniques Used to measure Rate of Reactions
Reaction between Fe3+ + I - can be measured using TWO different methods
Method 1 Method 2
Method 1
2Fe3+ + 2I - → 2Fe2+ + I2
Results
Research Questions possible
• As concentration increases ↑ , rate increases ↑
• Effect of Temperature and Concentration on the rate of reaction
• What is the order of reaction with respect to Fe3+ and I - concentration ?
Fe 3+ - Oxidising Agent I - - Reducing Agent
Techniques Used to measure Rate of Reactions
Reaction between Fe3+ + I - can be measured using TWO different methods
Method 1 Method 2
Method 2
• Rate of reaction measure as Δ in concentration of I2 or Increase in I2 concentration over time
• Apparatus is set up shown below
• 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- → S406
2- + 2I – ( Mole ratio is 1:2)
• Perform titration until volume of S2O32- added remains constant (Conc I2 produced remains constant)
Procedure
2Fe3+ + 2I - → 2Fe2+ + I2
Fe 3+ - Oxidising Agent I - - Reducing Agent
Techniques Used to measure Rate of Reactions
Reaction between Fe3+ + I - can be measured using TWO different methods
Method 1 Method 2
Method 2
2Fe3+ + 2I - → 2Fe2+ + I2
Results
Calculations
• At time 5mins – Vol of S2032- is 6.0ml – Amt of S203
2- = M x V = 0.2 x 0.006 = 0.0012mol
For 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
Fe 3+ - Oxidising Agent I - - Reducing Agent
Techniques Used to measure Rate of Reactions
Reaction between I2 + CH3COCH3 can be measured using TWO different methods
Method 1 Method 2
Method 1
• Rate of reaction measure as Δ in absorbance or Decrease in absorbance due to iodine
• Apparatus is set up shown below
• 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 λ max for I2 (λ 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 λ 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 .
Procedure
I2 + CH3COCH3 → CH3COCH2I + H+ + I -
Techniques Used to measure Rate of Reactions
Reaction between I2 + CH3COCH3 can be measured using TWO different methods
Method 1 Method 2
Method 1
I2 + CH3COCH3 → CH3COCH2I + H+ + I -
Results
Research Questions possible
• As concentration CH3COCH3 increases ↑ , decrease in absorbance over time increases ↑ , rate increases ↑
• Effect of Temperature and Concentration on the rate of reaction
• What is the order of reaction with respect to H+, CH3COCH3 and I2 concentration ?
Techniques Used to measure Rate of Reactions
Reaction between I2 + CH3COCH3 can be measured using TWO different methods
Method 1 Method 2
Method 2
• Rate of reaction measure as Δ in absorbance or Decrease in concentration of iodine
• 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 λ max for I2 (λ max = 520nm)
• Set colorimeter to Absorbance vs Concentration mode. (Standard calibration curve)
• Prepare a standard calibration curve for Absorbance vs I2 concentration shown below
Procedure
I2 + CH3COCH3 → CH3COCH2I + H+ + I -
•Pipette 0.4ml of I2, 0.4ml of 2M HCI and 1ml water into a cuvette. Start data collection at λ 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 .
Techniques Used to measure Rate of Reactions
Reaction between I2 + CH3COCH3 can be measured using TWO different methods
Method 1 Method 2
Method 2
I2 + CH3COCH3 → CH3COCH2I + H+ + I -
Results
Research Questions possible
• As concentration CH3COCH3 increases ↑ , decrease in absorbance over time increases ↑ , rate increases ↑
Convert Absorbance I2 to Concentration I2
using standard calibration curve
• Effect of Temperature and Concentration on the rate of reaction
• What is the order of reaction with respect to H+, CH3COCH3 and I2 concentration ?