The Temperature of the substance – When the temperature of the solution of reacting particles are increased, the particles will move quicker, so there is a higher chance of them colliding
Using a catalyst – As mentioned above, the catalyst gives the particles a surface to stick to so they can collide easier.
Using an enzyme (biological catalyst) – Basically the same as a catalyst, only this is biologically produced so it can never run out so long as there are living things.
Increasing the concentration in the substance – This occurs in a solution, and means that when there is less water, there is more chance of the reacting particles to collide with one another.
Increasing the amount of pressure of the gases – This is in a gas, and this means that when there is more pressure, the particles are more squashed together, so there is more chance of particles colliding.
Increasing the surface area of the reactant – If a solid breaks up into smaller pieces in a solution, then it will break down faster, as the reactant has more space to work on so more collisions would be able to take place at once.
Concentration
Line 1) this shows a slow reaction, one with a dilute solution.
Lines 2 and 3) these show a reaction going faster, with the amount of
Concentration high.
Line 4) this is the fastest reacting substance, and should be
the one with the highest concentration.
*Diagram and statements quoted from CGP Chemistry revision guide.
The concentration of a solution is when there is a greater amount of reactant than water (which in this case is that there may be more Hydrogen Peroxide), and the opposite is how dilute a solution may be. It is basically the same thing as pressure, but pressure applies for a gas state reaction, where as the concentration applies for a liquid state reaction.
To decrease the concentration of a solution, you must add more water to it, but to increase the concentration you must either add less water or none at all. When a solution is of thick concentration, the particles in that solution is more closely packed up, much like the atoms of a solid but with more spaces. The concentration of air is when pressure builds on the gases and the particles are squashed together in a tight narrow area. This is shown by how different solutions can be made concentrated or dilute:
Experiment
I chose to experiment with the concentration of the solution. I think that a highly concentrated solution will react faster as when a substance is highly concentrated, the particles inside it move closer together, therefore making it easier for them to collide and collide quicker.
To perform this experiment, I will need to use Hydrogen Peroxide (H2O2), the Catalyst Lead Oxide (PbO, in its powder form), Water (H2O), conical flask, two small measuring cylinders, A Eudiometer Tube (going up in cm ), a delivery tube, a large cube-shaped container, a stop-clock, measuring scales and a paper.
To do this experiment, I will measure out the Hydrogen Peroxide and Water in each of the small measuring cylinders. Then I’ll fill the container until just over the half mark with water. I shall then place the lead oxide, whilst on the paper on top of the scales and measure out 5cm of it. Then, I will add the Lead Oxide, Hydrogen Peroxide and Water together into the conical flask, put the delivery tube on top and put the end of the tube into the water. Then I’ll put the Eudiometer tube, filled with water, upside down into the water and over the end of the glass tube. As soon as that’s done, I’ll see how much oxygen is collected in one minute. When I have added the solutions together, I will shake the conical flask slightly so that the particles can move.
To keep this experiment being a fair test, I shall keep the amount of Lead Oxide the same, I will only raise up the amount of water by 10cm every time as well as reducing the amount of Hydrogen Peroxide by 10cm every time. I shall also use the same size measuring cylinders to measure the substances, and I will try to keep the amount of water in the Eudiometer Tube the same. I will also do my best to keep the temperature of the substances the same.
In this experiment, I will need to use different types of safety. I will need to keep a safe distance when pouring the solutions into the different containers, and also, make sure no substances spill out. I will also be using safety goggles in case of any solution splashing upward.
I will need to measure the two different substances in two different measuring cylinders of the same height, width and volume. The Hydrogen Peroxide will gradually reduce by 10cm each time round, starting from 50cm down to 10cm . Also, as the Hydrogen Peroxide is being reduced, the water should be measured and increased by 10cm each time round, starting from 0cm and going up to 40cm . I will keep the amount of Lead Oxide at 5g every time round. I will also measure the amount of water in the Eudiometer tube, just to make it more accurate. To keep the results the same and see if the results I get are good, I will repeat the experiment again, so it will be done two times in total.
Conclusion:
Through my results, I have discovered that the more concentrated a solution is, the more it will react when a catalyst is added to it. The results for when the concentration of Hydrogen Peroxide is 50cm with no water added is 33.0 and 32.05 respectively, and you can see this is a much larger reaction to the results of 10 cm Hydrogen Peroxide with 40 cm water, which were a measly 2.4 and 2.6. Through my scientific knowledge and understanding of the collision theory, I think this was due to the fact that when the catalyst was added, the reactant particles became ‘attached’ to the surface of the catalyst, and then collided strongly with the other particles to cause the reaction. The particles may have also collided strongly when going toward the surface of the catalyst. Because of the catalyst added, there is a lower activation energy needed for the particles to react with one another, so the reaction is able to occur easier and more frequent.
The graph above in the results shows the average amounts of Oxygen collected in the Eudiometer tube. As you can see, a line of best fit is drawn in to show a more accurate curved line. The steeper a line is, the more of a reaction has occurred. This is because of the relationship between the two subjects at hand, which in this case is Oxygen evolved against the concentration of the Hydrogen Peroxide. On the graph, it shows that there is a steeper line between the points at 40 and 50 than at the line between the points 10 and 20, showing that more reaction does occur with a higher concentration. When a reaction is faster, it is shown more higher and steeper on the chart, so when it becomes more steep towards the 50cm of Hydrogen Peroxide you know that 50cm of H2O2 is more effective than 10.
Evaluation
This experiment was difficult in the beginning, as we found some difficulties with the apparatus. The first time we tried the experiment, the apparatus turned out faulty, and we did not realise until we had already done it three or four times. The delivery tube was not keeping all the gas inside the flask and the actual tube, letting the Oxygen out in some part. When we solved that problem, everything else seemed fine, apart from one or two other mishaps, such as bad timing on the stop watch and the Eudiometer tube not being full to the brim of water, as some had spilt out into the large cube shaped container. I also found some of the measuring hard as the numbers had slightly rubbed off of the tube. I did find the capturing of the evolved Oxygen very easy, as I just simply needed to put the Eudiometer tube over the delivery tube. Getting the Eudiometer tube in the water was more difficult, as when I turned the Eudiometer tube upside down, some water sometimes fell out.
Next time I do this experiment, I would change the amount of Hydrogen Peroxide to reduce and Water to increase by 5cm , not 10 . I would also get properly marked measuring cylinders and Eudiometer tube. I would also try even more to keep the temperature the same, as we were working next to people using Bunsen burners.
All my results in the first experiment were correspondent with the repeated experiments results, so at least they were all around the same number. The only result that wasn’t ‘in line’ was the first result of the second experiment, as the second experiments’ results were slightly higher than the first experiments’ apart from that one.
To extend and improve this experiment, I could do a number of things. These include changing Lead Oxide to a different catalyst or maybe the same catalyst but in a pellet or gauze form, just to show a varied result. Also, I could change the experiment slightly by using a gas syringe connected to the delivery tube, so then there would be no need for the Eudiometer tube and the large container filled with water. The gas syringe would also help in accuracy, as it is already marked and has the same volume all around (the end of the Eudiometer tube is rounded and may affect the volume of Oxygen evolved being shown).
Bibliography
CGP revision guide to chemistry
“Chemistry Counts” textbook
www.askjeeves.com