Reaction Rate Investigation

I think this because of the collision theory. In the collision theory it states that in order for two substances to react together they must collide with each other and they must have enough energy.

Procedure-

Variables-

Diagram-

Materials-

• 25 ml graduated cylinder
• 100 ml graduated cylinder
• Stopwatch
• Stopper
• Plastic tube
• Side- arm test tube
• Calcium carbonate with large(powder), medium(small chips) and small(large chips) surface areas
• 1 mol l-1 of hydrochloric acid

Method-

1. Set up the apparatus as shown in the diagram.
2. Break the magnesium (Mg) into small pieces.
3. With a 25 ml graduated cylinder, measure out 5 ml of 1 mol l-1 hydrochloric acid(HCL).
4. Place the HCL into the test tube, while starting the stop watch.
5. Put the stopper on directly after you add the HCL
6. Collect the gas in the 100 ml graduated cylinder whit the tube form the side of the test tube.
7. Record the volume of as given off ever 20 seconds until it stops.

Results

Raw data-

Attached in Appendix I

Calculations-

Attached as Appendix II(written by hand)

Summary of results-

Graph-

Attached as Appendix III(by hand)

Conclusion-

When the surface area increases so does the rate of reaction.

This happens because the large surface area allows there to be more successful collisions, this ties into the collision theory mentioned in my hypothesis.

Evaluation-

Two Sources of Error-

• Temperature was not measures, instead it was referred to as “room temp”.
• The balance was only a two decimal point measure.

Problems with the method-

• Lost gas in the being form not sealing the tube fast enough

Suggestions to improve

• Look into better methods to keep gar from escaping.

What is a possible related investigation?-

• Choosing a different substance to react with HCL than the calcium carbonate.

Appendixes-

Appendix I- Full results