Investigate the rate of reaction between Calcium Carbonate and Hydrochloric Acid at different concentrations

Investigate the rate of reaction between Calcium Carbonate and Hydrochloric Acid at different concentrations

Aim:

To Investigate the rate of reaction between Calcium Carbonate and

Hydrochloric Acid at different concentrations.

Background Knowledge:

I know from my knowledge of science, that by adding together a carbonate and an acid, that a salt, water and Carbon Dioxide are produced. Therefore in order to measure the rate of reaction, one of these products needs to be measured, and the rate at which it is produced can be used to define the rate of the reaction. The methods that can be used are either to measure the mass of the solution at intervals. Or to measure the produce of gas (Carbon Dioxide).

Prediction:

Using the known formula:

ACID + CARBONATE SALT + CARBON DIOXIDE + WATER

I can predict the reaction of my experiment to be:

HYDROCHLORIC + CALCIUM à CALCIUM + WATER + CARBON

ACID CARBONATE CHLORIDE DIOXIDE

The Chemical Formula is listed below:

2HCl + CaCO3 CaCl2 + H20 + CO2

I think that as the molarity of the acid goes up, the amount of gas produced will also go up.

I have based this on my knowledge that calcium carbonate does not react in water. Therefore in solutions with little acid and more water, the calcium carbonate will not react as much as it would in pure acid for example. To make each of the different strengths of the acid, water is added to a solution of 2M hydrochloric acid. Therefore in the 0.2 value, there will be a lot of water, and so it is not expected that much gas will be produced.

My predicted graph shows what I expect. On the x-axis, as the molarity increases, the gas produced on the y-axis does likewise. However there will be a point reached where the maximum limit of gas has been prod... ... middle of paper ...

...a clear trend that as the molarity of the acid increases, the volume of carbon dioxide will also do the same.

There is an even trend going up, with a straight line to fit as the line of best fit.

The reason for this pattern is the same as that that was made in the prediction. As the concentration of the acid increases, there are more

HCl molecules and so there is more chance of the calcium carbonate molecules colliding with these and so reacting to form calcium chloride. With the reaction occurring more often, the products will form in a greater quantity and so more carbon dioxide is produced.

This reflects the rate of the reaction on the graph and proves my prediction and its theory correct.

Evaluation:

As the experiment was computer generated, it simulated how the experiment would have been conducted. It accounted for human errors in all aspects of the expriment.