Calcium carbonates (1g) During the experiment the equation I will be using is the following CaCO3 + 2HCL CaCL + H2O + CO2 If I use this formula each time then there should be a salt, the salt that is produced is Calcium Chloride. With this equipment I can plan my experiment, first I will measure out 100cm3 of hydrochloric acid and place it into a beaker, and I will then go and obtain 1g of calcium carbonate in which I will add to the beaker with the Hydrochloric acid.
When I do this I will then start the stop watch, I will then record my results every half minutes for the next 4 minuets and record my results. To make this a fair test I will use 100cm3 of Hydrochloric acid each time and only use 1g of calcium carbonate, but there is a problem in which I can not help, this is although the Calcium carbonate may weigh the same some of the Calcium carbonate might have a bigger surface area, this will then alter the experiment in some way.
If there is more surface area then there will be more reactions taking place because if there is a bigger surface area then there is more room for the molecules to collide with the calcium carbonate. Also I can not help the temperature, because if you are heating up your Hydrochloric acid then when you stop heating you could let out some of the heat, in turn causing the temperature to fall ever just so slightly which could affect the results just a bit, also when you measure out the hydrochloric acid you might not get all of the solution into the beaker causing it to have a slower reaction.
I predict that the hotter the solution is the more gas is given of, I think this because when the molecules gain lots of energy they soon start to move about, and when you get your molecules to move about there is a good chance of them colliding with the Calcium carbonate and when that happens you get a reaction taking place, so the hotter you heat the acid the more energy the molecules will causing likely hood of them causing a reaction is high, so therefore the reaction in which is taking place will speed up quite considerably.
I have chosen to do 5 experiments to see what will happen when you keep the temperature the same but change the concentration, each of the experiments will be taken over a 4 minute period, jotting down the amount of Carbon dioxide which is being given of every half minute. This action takes place when the Calcium Carbonate (CaCO3) touches the Hydrochloric acid (2HCL) the molecules then start reacting with the Calcium Carbonate (CaCO3)
Preliminary experiments We first before we did the experiment had to decide on how much concentration we would be using i.e. 90,100,110,120ml I then asked myself what temperatures would give me the greatest range of results, I thought that room temperature and at 50i?? would be good enough. Because if you go any higher than 70i?? the Hydrochloric acid will start to evaporate and would not be a fair test. Also time was a crucial thing because we did not have enough time to do 10, 15, 20 minutes, so I thought that a reasonable range of results would be around about 4 minutes, marking it down every half minute. Obtaining evidence.
During our experiment I made sure that I was working safely enough, for example: I wore my goggles at all times, I made sure that I was not running about, I made sure that I did not spill any Hydrochloric acid onto the floor. I collected a variable amount of results, in which will help me be able to produce a graph at the end, I have recorded my results in the table belowThese results were at room temperature the next ones are at 50i?? c:
Time 1As I predicted the hotter temperature is the faster reaction will be, because when the molecules in side the Hydrochloric acid are heated they gain more energy than the molecules that are at room temperature, when this happens then the molecules will have a great chance of colliding with each other, when this process happens the reaction will speed up. I think that one of our results were wrong because the hydrochloric acid stops producing Carbon dioxide and normally it will not do that.