Planning of Experiment

1. 1
SIZE OF REACTANT
Aim:
To investigate the effect of size calcium carbonate on the
rate of reaction
Problem Statement:
How does the size of calcium carbonate affect the rate of
reaction?
Hypothesis:
When the size of calcium carbonate smaller, the rate of
reaction increase/higher
Variables:
(a) Manipulated:
Size of calcium carbonate
(b) Responding:
Rate of reaction
(c) Constant:
Mass of calcium carbonate, volume and
concentration of hydrochloric acid
Apparatus:
Retord stand with clamp, burette, basin, conical flask,
delivery tube, stopper, stopwatch, measuring cylinder
Materials:
Water, calcium carbonate, hydrochloric acid
Procedure:
1. Fill a burette with water and invert it over water in a
basin.
2. Clamp the burette vertically using a retort stand.
Record its initial reading.
3. Measure 40 cm3
of 0.1 mol dm-3
hydrochloric acid, HCl
using a measuring cylinder and pour the acid into a
conical flask.
4. Weigh 2g of large marble chips (set I) and put into the
conical flask.
5. Close the conical flask immediately with a stopper
which is joined to the delivery tube
6. Start the stopwatch.
7. Shake the conical flask throughout the experiment.
8. Record the burette reading at intervals of 30 seconds
until the reaction stops.
9. Repeat steps 1 to 8 using 2g small marble chips (set II)
to replace 2g of large marble chips.
Tabulation of data:
Experiment Time (s) 0 30 60 90 120
1
Burette
reading (cm3
)
Total volume
of gas (cm3
)
2
Burette
reading (cm3
)
Total volume
of gas (cm3
)
PLANNING OF EXPERIMENT TO STUDY THE
FACTOR THAT AFFECT THE RATE OF REACTION

2. 2
CONCENTRATION OF SOLUTION
Aim:
To investigate the effect of concentration sodium
thiosulphate, Na₂S₂O₃ solution on the rate of reaction.
Problem Statement:
How does the concentration of sodium thiosulphate,
Na₂S₂O₃ solution affect the rate of reaction?
Hypothesis:
The higher the concentration of sodium thiosulphate,
Na₂S₂O₃ solution, the higher the rate of reaction.
Variables:
(a) Manipulated:
Concentration of sodium thiosulphate, Na₂S₂O₃
solution
(b) Responding:
Rate of reaction
(c) Constant:
Volume and concentration of sulphuric acid.
Apparatus:
Conical flask, 50 cm³ measuring cylinder, 10 cm³
measuring cylinder, stopwatch
Materials:
0.2 mol dm-3
sodium thiosulphate solution, 1.0 mol dm-3
sulphuric acid, distilled water, white paper marked ‘X’ at
the centre
Procedure:
1. Measure 50 cm3
of 0.2 mol dm-3
sodium thiosulphate,
Na2S2O3 solution using a measuring cylinder and pour it
into a conical flask.
2. Place the conical flask on top of a piece of white paper
marked ‘X’.
3. Measure 5 cm3
of 1.0 mol dm-3
sulphuric acid, H2SO4
using another measuring cylinder.
4. Pour the sulphuric acid, H2SO4 quickly and carefully into
the conical flask. At the same time, start the stopwatch.
5. Swirl the mixture in the conical flask.
6. Observe the ‘X’ mark vertically from the top of the
conical flask through the solution.
7. Stop the stopwatch once the ‘X’ mark disappears from
sight and record the time taken.
8. Repeat steps 1 to 7 using different concentrations of
sodium thiosulphate, Na2S2O3 solution.
Tabulation of data:
Experiment
Concentrations of
sodium
thiosulphate,
Na2S2O3 solution
(mol dm-3
)
Time taken for
‘X’ mark to
disappear from
sight, t (s)
1
2
3
4
5

3. 3
TEMPERATURE
Aim:
To investigate the effect of temperature sodium
thiosulphate solution on the rate of reaction.
Problem Statement:
How does the temperature sodium thiosulphate solution
affect the rate of reaction?
Hypothesis:
The higher the temperature sodium thiosulphate solution,
the higher the rate of reaction.
Variables:
(a) Manipulated:
Temperature of sodium thiosulphate solution
(b) Responding:
Rate of reaction
(c) Constant:
Volume and concentration of sodium thiosulphate
solution, volume and concentration of sulphuric
acid.
Apparatus:
Conical flask, measuring cylinder, stopwatch,
thermometer, Bunsen burner, tripod stand, wire gauze.
Materials:
0.2 mol dm-3
sodium thiosulphate solution, 1 mol dm-3
sulphuric acid, white paper marked ‘X’ at the centre
Procedure:
1. Measure 50 cm3
of 0.2 mol dm-3
sodium thiosulphate,
Na2S2O3 solution using a measuring cylinder and pour it
into a conical flask.
2. Place the conical flask on top of a piece of white paper
marked ‘X’.
3. Measure 5 cm3
of 1.0 mol dm-3
sulphuric acid, H2SO4
using another measuring cylinder.
4. Pour the sulphuric acid, H2SO4 quickly and carefully into
the conical flask. At the same time, start the stopwatch.
5. Swirl the mixture in the conical flask.
6. Observe the ‘X’ mark vertically from the top of the
conical flask through the solution.
7. Stop the stopwatch once the ‘X’ mark disappears from
sight and record the time taken.
8. Repeat steps 1 to 7 using 50 cm3
of 0.2 mol dm-3
sodium thiosulphate, Na2S2O3 solution at 40°C, 50 °C,
60°C and 70°C by heating the solution before adding in
5 cm3
of 1.0 mol dm-3
sulphuric acid, H2SO4.
Tabulation of data:
Experiment
Temperature
(°C)
Time taken for
‘X’ mark to
disappear from
sight, t (s)
1 28
2 40
3 50
4 60
5 70

4. 4
CATALYST [DECOMPOSITION OF HYDROGEN PEROXIDE]
Aim:
To investigate the effect of manganese(IV) oxide on the
rate of decomposition of hydrogen peroxide.
Problem Statement:
Does the presence of manganese(IV) oxide affect the rate
of decomposition of hydrogen peroxide?
Hypothesis:
The presence of manganese(IV) oxide will increase the rate
of decomposition of hydrogen peroxide.
Variables:
(a) Manipulated:
Presence of manganese(IV) oxide
(b) Responding:
Rate decomposition of hydrogen peroxide
(c) Constant:
Volume and concentration of hydrogen peroxide,
mass of manganese(IV) oxide
Apparatus:
Retord stand with clamp, burette, basin, conical flask,
delivery tube, stopper, stopwatch, measuring cylinder
Materials:
Water, hydrogen peroxide solution, manganese(IV) oxide
Procedure:
1. Fill a burette with water and invert it over water in a
basin.
2. Clamp the burette vertically using a retort stand.
Record its initial reading.
3. Measure 25 cm3
of hydrogen peroxide, H2O2 using a
measuring cylinder and pour into a conical flask.
4. Close the conical flask immediately with a stopper
which is joined to the delivery tube
5. Start the stopwatch.
6. Shake the conical flask throughout the experiment.
7. Record the burette reading at intervals of 30 seconds
until the reaction stops.
8. Repeat steps 1 to 7 by adding [1-5] g manganese(IV)
oxide into the hydrogen peroxide solution.
Tabulation of data:
Experiment Time (s) 0 30 60 90 120
1
Burette
reading (cm3
)
Total volume
of gas (cm3
)
2
Burette
reading (cm3
)
Total volume
of gas (cm3
)

5. 5
CATALYST [ZINC AND SULPHURIC ACID]
Aim:
To investigate the effect of copper(II) sulphate on the rate
of reaction between zinc and sulphuric acid.
Problem Statement:
Does the presence of copper(II) sulphate affect the rate of
reaction between zinc and sulphuric acid?
Hypothesis:
The presence of copper(II) sulphate will increase the rate
of reaction between zinc and sulphuric acid.
Variables:
(d) Manipulated:
Presence of copper(II) sulphate solution
(e) Responding:
Rate of reaction
(f) Constant:
Volume and concentration of sulphuric acid,
mass of zinc
Apparatus:
Retord stand with clamp, burette, basin, conical flask,
delivery tube, stopper, stopwatch, measuring cylinder
Materials:
Water, hydrogen peroxide solution, manganese(IV) oxide
Procedure:
1. Fill a burette with water and invert it over water in a
basin.
2. Clamp the burette vertically using a retort stand.
Record its initial reading.
3. Measure 25 cm3
of 0.1 mol dm-3
sulphuric acid using a
measuring cylinder and pour into a conical flask.
4. Close the conical flask immediately with a stopper
which is joined to the delivery tube
5. Start the stopwatch.
6. Shake the conical flask throughout the experiment.
7. Record the burette reading at intervals of 30 seconds
until the reaction stops.
8. Repeat steps 1 to 7 by adding a few drops of copper(II)
sulphate solution into the mixture of zinc and sulphuric
acid.
Tabulation of data:
Experiment Time (s) 0 30 60 90 120
1
Burette
reading (cm3
)
Total volume
of gas (cm3
)
2
Burette
reading (cm3
)
Total volume
of gas (cm3
)