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Hydrochloric acid and Marble Chips

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Hydrochloric acid and Marble Chips Aim The aim of this experiment is to find out how different variables affect the rate at which the reaction between Marble chips (CaCO ) and Hydrochloric acid (HCl) takes place. There are many variables that effect the rate of this reaction such as the following: 1. Temperature 2. Concentration (Pressure for gases) 3. Catalyst 4. Surface area In my investigation I will be testing how changing the concentration of the Hydrochloric acid makes an effect and changes the speed of the reaction. I will do various experiments and then evaluate the results and come to a conclusion. The reaction that will take place is Hydrochloric acid + Calcium Carbonate Calcium Chloride + Water + Carbon dioxide Hypothesis The more concentrated the acid then the quicker the reaction will take place, because there will be more HCl particles than water particles for the marble chips to collide with and therefore react. More collisions between the two reactants (HCl and CaCO) will take place resulting in a quicker time for the reaction. ...read more.


The activation energy is reduced so that there is a better chance of particles having enough energy to react. Reactants will need less energy to react. 2. The number and strength of collisions is increased so that the reaction can happen faster. If the particles have more energy then more particles will be able to react. Solid reactants like marble chips are effected by surface area, the larger the surface area the more collisions that will take place. This will increase the rate of reaction and decrease the time taken. Liquid/ Aqueous reactants rely on collisions for more collisions to take place. In a concentrated acid solution there are more acid particles so more collisions will take place. There will be an increase in the product formed in a certain time. When the temperature is increased, the particles will have more energy, so they will move faster. This will result in the particles colliding more frequently and increasing the speed of the reaction. Also when they have more energy there will be more chance of the collisions being successful because the activation energy will be attainable. ...read more.


A less or mare concentrated solution will be used but the total volume of the solution will stay the same. Evaluation The results show that the more concentrated the acid is then the faster the reaction happens. When there was 10 parts acid and no water, the reaction takes place much faster compared to when there was only 1 part acid and 9 parts water. I the reaction with concentrated acid 65 cm of carbon dioxide is produced in the first 10 seconds while only 3 cm of carbon dioxide is produced by using the least concentrated solution. There is no pattern as to how much of an increase there is because when the concentration is doubled from 5:5 to 10:0. The amount of carbon dioxide produced in the first 10 seconds doesn't double but goes from 17 to 65 which is more than triple. These results are not very accurate and can be improved. If the experiment is done twice and the average is taking the results will be more accurate. Conclusion Overall the results obtained were quite accurate and showed that an increase in the concentration of the acid means that the rate of the reaction increases and the time taken is decreased. ...read more.

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