Effect Of Catalyst On The Rate Of Reaction Teacher’s Guide/
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EFFECT OF CATALYST ON THE RATE OF REACTION Teacher’s Guide/ Chemistry Form 5/ Spreadsheet SCIENTIFIC CONCEPT Rate of reaction is the speed at which reactants are converted into the products in a chemical reaction. For the reaction that occurs rapidly, the rate of reaction is high. Conversely, for a reaction that occurs slowly, the rate of reaction is low. The time taken for a fast reaction is short, whereas the time taken for a slow reaction is long. Hence, the rate of particular reaction is inversely proportional to the time taken for the reaction. One of the factors that can be affecting the rate of reaction is catalyst. A catalyst is a substance which can alter the rate of a chemical reaction while itself remains chemically unchanged at the end of the reaction. The effect of the amount of catalyst on the rate of reaction can be determine by comparing two experiment. The first experiment is the rate of reaction by using 0.2g of manganese (IV) oxide powder. While, the second experiment is rate of reaction by using 0.8g of manganese (IV) oxide powder. When the amount of a catalyst used increases, the rate of reaction also increases. Experiment 1: The rate of reaction by using 0.2g of manganese (IV) oxide powder. Time (s) Burette
0 48.60
reading (cm3) Volume of 0.00 oxygen
30 42.00
60 36.10
90 30.70
120 25.60
150 21.20
180 16.80
210 13.40
240 9.95
6.60
12.50
17.90
23.00
27.40
31.80
35.20
38.65
gas
liberated (cm3)
Experiment 2: The rate of reaction by using 0.8g of manganese (IV) oxide powder. Time (s) Burette
0 49.30
reading (cm3) Volume of 0.00 oxygen
30 40.55
60 34.30
90 28.30
120 23.10
150 18.35
180 14.20
210 10.30
240 6.90
8.75
15.00
21.00
26.20
30.95
35.10
39.00
42.40
gas
liberated (cm3) UNIQUE FEATURE OF THIS ACTIVITY
• The data can be manipulated easily, for example every 30 second, the level of water in the burette was taken. • Data displayed in a systematic manner, save time in drawing graph, show relationship of the volume of oxygen gas liberated against time for both experiment on the same axes. • Student will discover that a spreadsheet can be used to process data. • Allow the student to do more important things such as analyzing the data or the graph.
ENGAGE
You are given two different pictures. Observe the picture carefully.
( A)
What can you observe from the picture? Based on the picture, which one is moving faster?
EMPOWER
(B)
Step 1.
2.
Student are given: •
50 cm³ measuring cylinder
•
150 cm³ conical flask
•
Stopper with delivery tube
•
Burette
•
Retort stand and clamp
•
Basin
•
Electronic balance
•
Stopwatch
•
Spatula
•
Beaker
•
2-volume hydrogen peroxide solution
•
Manganese (IV) oxide powder
Student needs to plan an experiment to determine the effect of catalyst on the rate of reaction.
3.
Student has to construct a hypothesis for this experiment.
4.
Student should know the effect of catalyst of the reaction.
5.
Help student to determine the variables involved.
6.
You may give these instructions to start the activity:
Open a spreadsheet file
Name the file as ‘the effect of catalyst on the rate of reaction’
Fill a burette with water until it is full. Invert the burette over water in a basin and clamped vertically using a retort stand. Adjust the water level in the burette and record the initial reading of burette. By using a measuring cylinder, measure 50 cm³ 0f 2 volume hydrogen peroxide solution and pour it into a conical flask. Weight 0.2g of manganese (IV) oxide powder by using an electronic balance and poured carefully into a conical flask. Close the conical flask immediately with stopper fit with a delivery tube direct to the burette. At the same time, immediately start the stopwatch. Shake the conical flask with its content slowly and record the volume of oxygen gas collected in the burette at regular intervals of 30 seconds for 4 minutes. Repeat the procedure by using 0.8g manganese (IV) oxide powder. How to set up the spreadsheet 1. Insert the data that obtain from the experiment to the table 2. Insert the border in the table.
How to draw a graph with the spreadsheet 1. Select a line graph 2. Highlight B4 to K4, click ‘Series’, this will draw a line graph base the data from the highlight area that is concentration versus time taken. 3. Click ‘category(x) axis’ label, highlight C4 to K4 (this will show the actual scale of xaxis according to the data), then click ‘Next’. 4. Name the chart 5. Label the x-axis and y-axis as time and volume of gas oxygen liberated.
6. Apply the same step to draw the second graph, volume of gas oxygen liberated versus time.
RESULTS: Experiment 1: The rate of reaction by using 0.2g of manganese (IV) oxide powder. Time (s) Burette
0 48.60
30 42.00
60 36.10
90 30.70
120 25.60
150 21.20
180 16.80
210 13.40
240 9.95
6.60
12.50
17.90
23.00
27.40
31.80
35.20
38.65
reading (cm3) Volume oxygen
of 0.00 gas
liberated (cm3)
Experiment 2: The rate of reaction by using 0.8g of manganese (IV) oxide powder. Time (s) Burette
0 49.30
30 40.55
60 34.30
90 28.30
120 23.10
150 18.35
180 14.20
210 10.30
240 6.90
8.75
15.00
21.00
26.20
30.95
35.10
39.00
42.40
reading (cm3) Volume oxygen
of 0.00 gas
liberated (cm3)
volume of oxygen gas liberated (cm3)
graph of volume of oxygen gas liberated against time 45 40 35 30 25 20 15 10 5 0
0.2g manganese (IV) oxide 0.8g manganese (IV) oxide
0
100
200
300
time (s)
QUESTION: 1.
Which the reactant that having the highest the rate of reaction?
2.
What type of catalyst that we use in this experiment? Why?
3.
What type of gas formed in the burette?
ANSWER: 1.
0.8g manganese (IV) oxide powder.
2.
Positive catalyst because the catalyst increases the rate of reaction.
3.
Oxygen gas
ENHANCE
A= wash with small amount of detergent
B= wash with large amount of detergent
When both plates are washed, which one is faster to clean? Explain.
ANSWER: Plate B will clean first. It is because detergent like a catalyst will clean the plate easily due to the large amount of detergent that used. The larger amount of detergent used will increase the rate of reaction between oil and detergent.
0 48.60
reading (cm3) Volume of 0.00 oxygen
30 42.00
60 36.10
90 30.70
120 25.60
150 21.20
180 16.80
210 13.40
240 9.95
6.60
12.50
17.90
23.00
27.40
31.80
35.20
38.65
gas
liberated (cm3)
Experiment 2: The rate of reaction by using 0.8g of manganese (IV) oxide powder. Time (s) Burette
0 49.30
reading (cm3) Volume of 0.00 oxygen
30 40.55
60 34.30
90 28.30
120 23.10
150 18.35
180 14.20
210 10.30
240 6.90
8.75
15.00
21.00
26.20
30.95
35.10
39.00
42.40
gas
liberated (cm3) UNIQUE FEATURE OF THIS ACTIVITY
• The data can be manipulated easily, for example every 30 second, the level of water in the burette was taken. • Data displayed in a systematic manner, save time in drawing graph, show relationship of the volume of oxygen gas liberated against time for both experiment on the same axes. • Student will discover that a spreadsheet can be used to process data. • Allow the student to do more important things such as analyzing the data or the graph.
ENGAGE
You are given two different pictures. Observe the picture carefully.
( A)
What can you observe from the picture? Based on the picture, which one is moving faster?
EMPOWER
(B)
Step 1.
2.
Student are given: •
50 cm³ measuring cylinder
•
150 cm³ conical flask
•
Stopper with delivery tube
•
Burette
•
Retort stand and clamp
•
Basin
•
Electronic balance
•
Stopwatch
•
Spatula
•
Beaker
•
2-volume hydrogen peroxide solution
•
Manganese (IV) oxide powder
Student needs to plan an experiment to determine the effect of catalyst on the rate of reaction.
3.
Student has to construct a hypothesis for this experiment.
4.
Student should know the effect of catalyst of the reaction.
5.
Help student to determine the variables involved.
6.
You may give these instructions to start the activity:
Open a spreadsheet file
Name the file as ‘the effect of catalyst on the rate of reaction’
Fill a burette with water until it is full. Invert the burette over water in a basin and clamped vertically using a retort stand. Adjust the water level in the burette and record the initial reading of burette. By using a measuring cylinder, measure 50 cm³ 0f 2 volume hydrogen peroxide solution and pour it into a conical flask. Weight 0.2g of manganese (IV) oxide powder by using an electronic balance and poured carefully into a conical flask. Close the conical flask immediately with stopper fit with a delivery tube direct to the burette. At the same time, immediately start the stopwatch. Shake the conical flask with its content slowly and record the volume of oxygen gas collected in the burette at regular intervals of 30 seconds for 4 minutes. Repeat the procedure by using 0.8g manganese (IV) oxide powder. How to set up the spreadsheet 1. Insert the data that obtain from the experiment to the table 2. Insert the border in the table.
How to draw a graph with the spreadsheet 1. Select a line graph 2. Highlight B4 to K4, click ‘Series’, this will draw a line graph base the data from the highlight area that is concentration versus time taken. 3. Click ‘category(x) axis’ label, highlight C4 to K4 (this will show the actual scale of xaxis according to the data), then click ‘Next’. 4. Name the chart 5. Label the x-axis and y-axis as time and volume of gas oxygen liberated.
6. Apply the same step to draw the second graph, volume of gas oxygen liberated versus time.
RESULTS: Experiment 1: The rate of reaction by using 0.2g of manganese (IV) oxide powder. Time (s) Burette
0 48.60
30 42.00
60 36.10
90 30.70
120 25.60
150 21.20
180 16.80
210 13.40
240 9.95
6.60
12.50
17.90
23.00
27.40
31.80
35.20
38.65
reading (cm3) Volume oxygen
of 0.00 gas
liberated (cm3)
Experiment 2: The rate of reaction by using 0.8g of manganese (IV) oxide powder. Time (s) Burette
0 49.30
30 40.55
60 34.30
90 28.30
120 23.10
150 18.35
180 14.20
210 10.30
240 6.90
8.75
15.00
21.00
26.20
30.95
35.10
39.00
42.40
reading (cm3) Volume oxygen
of 0.00 gas
liberated (cm3)
volume of oxygen gas liberated (cm3)
graph of volume of oxygen gas liberated against time 45 40 35 30 25 20 15 10 5 0
0.2g manganese (IV) oxide 0.8g manganese (IV) oxide
0
100
200
300
time (s)
QUESTION: 1.
Which the reactant that having the highest the rate of reaction?
2.
What type of catalyst that we use in this experiment? Why?
3.
What type of gas formed in the burette?
ANSWER: 1.
0.8g manganese (IV) oxide powder.
2.
Positive catalyst because the catalyst increases the rate of reaction.
3.
Oxygen gas
ENHANCE
A= wash with small amount of detergent
B= wash with large amount of detergent
When both plates are washed, which one is faster to clean? Explain.
ANSWER: Plate B will clean first. It is because detergent like a catalyst will clean the plate easily due to the large amount of detergent that used. The larger amount of detergent used will increase the rate of reaction between oil and detergent.
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