Rate of reaction between calcium carbonate and hydrochloric acid.

Andrew Mckean

Rate of reaction coursework

Calcium carbonate reacts with hydrochloric acid producing calcium chloride, water and carbon dioxide.

CaCO3(s)+ 2HCl (aq) ----- CaCl (aq)+ H2O (L)+CO2 (g)

Theory

The things that could affect the rate of the reaction are surface area, concentration, temperature and catalyst. I will change the concentration of the HCl this should prove that the reaction of the HCl with calcium carbonate should be slower if the HCL is more concentrated.

Prediction

In my experiment I will predict that when I change the concentration of the hydrochloric acid the rate of the reaction will increase, because there is more acid then there will be more collisions therefore there will be more gases coming of the limestone, if I start to add water to the hydrochloric acid the rate of the reaction will be slower because their will be less collisions of the molecules. I will change the concentration of the acid by adding water to it. This will be the one that I am going to change because it will be easy and accurate.

If I increased the surface area of the limestone by chopping if up there rate of the reaction will be increased because the is more molecules to collide with.

If I made a catalyst the rate of the reaction would also be quicker because a catalyst makes a shortcut in the reaction therefore the reaction will be quicker.

If I increase the temperature of the water the rate of the reaction would also be quicker because there would be more energy in the molecules and there would be more collisions, therefore they will react with each other quicker.

Method ...

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If I increased the surface area of the limestone by chopping if up there rate of the reaction will be increased because the is more molecules to collide with.

If I made a catalyst the rate of the reaction would also be quicker because a catalyst makes a shortcut in the reaction therefore the reaction will be quicker.

Method

First I set up all my equipment and the I measured out all the amounts of acid and water that I was going to use, I got a bowl of water and put the beehive shelf in it, on top of the beehive shelf I put a tube upside down on top of I full of water, then in a test tube I put 5gs of limestone rock and 25ml of HCL then from the test tube I put a bung with a tube from it into the beehive shelf so that the bubbles produced would go into the large test tube with water in it so that I could measure that amount of gas that has come of it. I repeated the test 3 times so that I had there different sets of results each time I decreased the amount of HCL by 5ml and increased the amount of water by 5ml so that I would have different concentrations of water.

Results

In my first set of results I used, 2ml HCL, 0ml water, 5g Limestone.
In my second set of results I used, 20ml HCL, 5ml Water, 5g Limestone.
In my third set of results I used, 15ml HCL, 10ml Water, 5g Limestone.

Evaluation

I think that my experiment was successful because everything went to plan and I got the results that I expected so this meat that my write up would not be difficult. If I did the experiment again I would change the amounts of acid and water that I used so that I could get more results and therefore make a better graph. I would also use a syringe o catch the bubbles in so that my results would be even more accurate. I could have also used the HCl all from the same bottle because the strengths of the acid could have been slightly different even though it said on the bottle because somebody could have put some water in the bottle before therefore my results could have been wrong.

Conclusion

By doing the experiment I have proved that my theory is right. It has shown that the concentration of the HCl does effect the rate of the reaction because when the acid is less concentrated then the rate of the Reaction will be slower you can see that there is less gasses produced in a given time.