Rates of Reaction

Experiment 1:
Investigating the effect of temperature on reaction rate

Aim:
I want to investigate how temperature effects the reaction rate.

Equipment

• Conical Flask
• Beaker
• Measuring Cylinder
• Stopwatch
• Waterbath
• Paper with a black cross "X"
• Thermometer
• 0.1mol/L Sodium Thiosulfate
• 2.0mol/L Hydrochloric Acid

Method:

1. Put the piece of paper with the X on the bench and put the conical flask on it
2. Measure 50mL of Sodium Thiosulfate and put it into a beaker.
3. Record the temperature of the Sodium Thiosulfate.
4. Measure 5mL of HCl and put it into the conical flask.
5. Pour the Sodium Thiosulfate into the conical flask, start the timer and swirl the flask.
6. Stop timing when the you can't see the cross on the paper
7. Wash out the flask thoroughly.
8. Repeat the experiment with the Sodium Thiosulfate at 30°C .
9. Repeat the experiment with the Sodium Thiosulfate at 40°C .
10. Repeat the experiment with the Sodium Thiosulfate at 50°C

Results:

17°C  took 33sec for the X to disappear.
32°C  took 21sec for the X to disappear.
43°C  took 7sec for the X to disappear.
57°C  took 2sec for the X to disappear.

Analysis:

Conclusion:

Collision theory is for a reaction to occur two or more particles must collide with sufficient force and the correct orientation. By increasing the temperature of the particles it makes them move faster, increasing the chance of them colliding quicker.

Experiment 2:

Investigating the effect of concentration on reaction rate

Aim:
I want to investigate how concentration effects the reaction rate.

Equipment

• Conical Flask
• Beaker
• Measuring Cylinder
• Stopwatch
• Waterbath
• Paper with a black cross "X"
• Thermometer
• 0.1mol/L Sodium Thiosulfate
• 2.0mol/L Hydrochloric Acid

Method:

1. Put the piece of paper with the X on the bench and put the conical flask on it
2. Measure 10mL of Sodium Thiosulfate and put it into the conical flask
3. Measure 40mL of Water and put it into the conical flask. Swirl to mix.
4. Measure 5mL of HCl.
5. Pour the HCl into the conical flask, start the timer and swirl the flask.
6. Stop timing when the you can't see the cross on the paper.
7. Wash out the flask thoroughly.
8. Repeat experiment 20mL of Sodium Thiosulfate and 30mL of Water.
9. Repeat experiment 30mL of Sodium Thiosulfate and 20mL of Water.
10. Repeat experiment 40mL of Sodium Thiosulfate and 10mL of Water.
11. Repeat experiment 50mL of Sodium Thiosulfate and no Water

Results:

10mL Thiosulfate/40mL Water took 239sec for the X to disappear.
20mL Thiosulfate/30mL Water took 119sec for the X to disappear.
30mL Thiosulfate/20mL Water took 64sec for the X to disappear.
40mL Thiosulfate/10mL Water took 45sec for the X to disappear.
50mL Thiosulfate/0mL Water took 32sec for the X to disappear.

Analysis:

Conclusion:

Collision theory is for a reaction to occur two or more particles must collide with sufficient force and the correct orientation. By increasing the concentration it means there are more particles and their closer together so they have a better chance at colliding.

Experiment 3:
Investigating the effect of surface area on reaction rate

Aim:
I want to investigate how changing the surface area effects the reaction rate.

Equipment

• Boiling Tube
• Calcium Carbonate (Marble) Chips
• Calcium Carbonate Powder
• 1.0mol/L Hydrochloric Acid
• Measuring cylinder
• Spatula
• Test tube tongs

Method:

1. Measure 2mL of Hydrochloric Acid and pour it into a boiling tube.
2. Using the tongs to hold the boiling tube tube the sink, add a pea-sized amount of Calcium Carbonate powder.
3. Repeat experiment instead using the same amount of marble chips rather than the powder. 

Results:

When I added the powder, there was vigorous fizzing.
When I repeated the experiment with the chips, it bubbled

Conclusion:

Collision theory is for a reaction to occur two or more particles must collide with sufficient force and the correct orientation. If a reactant is broken into little pieces, it has a bigger surface area making the particles more exposed meaning more of them can collide.

Experiment 4:
Investigating the effect of a catalyst on the reaction rate 

Aim:
I want to investigate how adding a catalyst will effect the reaction rate.

Equipment

• 3x test tubes
• Zinc metal granules
• Copper metal powder
• 1.0mol/L Hydrochloric Acid
• Measuring cylinder
• Spatula

Method:

1. Put a piece of zinc into test tube 1 and test tube 3.
2. Put a small amount of copper powder to test tube 2 and test tube 3.
3. Add 5mL of acid to each test tube.

Conclusion: 

A catalyst a substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change.