• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

I am going to see how long it will take the Calcium carbonate to neutralise the acid at different temperatures, I am going to see what will happen to the speed of reaction when I change the temperature

Extracts from this document...


Plan I am going to see how long it will take the Calcium carbonate to neutralise the acid at different temperatures, I am going to see what will happen to the speed of reaction when I change the temperature, and then I will see how much Carbon dioxide is produced over a period of time. The equipment that I am going to use is the following: Beaker Tub full of water Measuring cylinder Pipe to connect the two Stop watch Bunsen burner Tri pod Thermometer Clamp 100cm3 hydrochloric acid 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. ...read more.


I think that one of our results were wrong because the hydrochloric acid stops producing Carbon dioxide and normally it will not do that. Here is the result that was wrong and also the repeated results: Time 1g/0.5m 0 0 cm3 0.5 1 cm3 1 2 cm3 1.5 3 cm3 2 3 cm3 2.5 4 cm3 3 5 cm3 3.5 5 cm3 4 6 cm3 Repeated results: Time 1g/0.5m 0 0 cm3 0.5 1 cm3 1 2 cm3 1.5 4 cm3 2 5 cm3 2.5 6 cm3 3 7 cm3 3.5 8 cm3 4 9 cm3 These repeated results are better because there is a following pattern of how much Carbon dioxide is being produced, instead of the Carbon dioxide starting and stopping. My results are not that reliable because I did not have enough time to extend the amount of time given to make my results more accurate. If I had the time I would have gone for 10 or 15 minutes this would have given me a greater range of results to prove that when you heat the hydrochloric acid the reaction is faster and you will get greater results to draw from. There are many problems with the experiment, the first is the Calcium carbonate, you might have think you have got 1g of Calcium carbonate but the surface area might be bigger, with this ...read more.


the answer to this could have been that the surface area of the Calcium carbonate could have been smaller or bigger for the molecules to collide with the Calcium Carbonate. To make sure that my conclusion was right I could have done the experiment again and tested my theory of molecules colliding to make the reaction happen faster. Theory used to predict the rates of chemical reactions, particularly for gases. The collision theory is based on the assumption that for a reaction to occur it is necessary for the reacting species (atoms or molecules) to come together or collide with one another. Not all collisions, however, bring about chemical change. A collision will be effective in producing chemical change only if the species brought together possess a certain minimum value of internal energy, equal to the activation energy of the reaction. Furthermore, the colliding species must be oriented in a manner favourable to the necessary rearrangement of atoms and electrons. Thus, according to the collision theory, the rate at which a chemical reaction proceeds is equal to the frequency of effective collisions. I could have also changed the amount of 2HCL that I used to prove that when you heat the Hydrochloric acid (2HCL) and use however much concentration you use that as soon as you heat it up you will always get better results in the end. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Patterns of Behaviour essays

  1. Marked by a teacher

    In this project I am going to investigate rates of reaction of an indigestion ...

    3 star(s)

    Collisions between molecules are stronger at higher temperatures. In an ineffective reaction, the molecules just rebound off each other. My Experiment I am going to investigate the relationship between rates of reaction and temperature. I chose temperature because it is easy to keep the concentration constant and from previous experiments

  2. Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

    I will show how I plan to get my results, I will show my method in a step-by-step way: 1. Take the cone shaped conical flask. 2. Measure 50cm3 of 1 molar hydrochloric acid in a measuring cylinder. Keep the cylinder on the table and bend your knees to keep an eye on the volume of acid.

  1. The Reaction Between Calcium Carbonate and Hydrochloric Acid

    This makes it more likely that the collisions contain the minimum activation energy. Yet again this is another way of increasing the chance of creating more successful collisions, which means a faster rate of reaction. Fig. 2.a Increasing Temperature As you can see from the above graph, figure 2.b, the

  2. The variable that I will change will be the temperature of the water that ...

    I stopped timing and wrote down the time gained in my results table. * A thermometer was placed in the beaker of water to measure the temperature (�C) of the water until the required temperature is reached. I made sure not to place it in the beaker while being heated.

  1. I am going to investigate the rate of reaction between calcium carbonate and hydrochloric ...

    This diagram shows many particles, indicating a high concentration. This has a high chance of chemical reaction, as there is little space to move without colliding with another particle. This causes the high chance of collision and chemical reaction, and shows that the higher the concentration, the more chemical reactions will take place.

  2. Investigating rates of reaction with the amount of carbon dioxide produced when various concentrations ...

    They cannot get over the top of the activation energy barrier so they fall back, still as reactants, regaining their original kinetic energy. On the other hand, if the combined kinetic energies of the reactants are equal to or greater than EA and the molecules are correctly orientated, they can overcome the activation energy barrier and form product molecules.

  1. Investigating the rate of reaction between hydrochloric acid and calcium carbonate

    acid 1gram = 1000 x 36.5 = 0.0365 we are able to tell that : 1cm3 = 0.0365 The smallest amount of Hydrochloric acid used in this experiment was 20ml so to calculate the amount of calcium carbonate = 0.0365 x 20 = 0.73g but because this is too big we found that using 0.4 would be the best option.

  2. An Investigation: Factors That Affect The Rate Of Reaction between Calcium carbonate and Hydrochloric ...

    In this Table there does not seem to be any out liners which is a good start for the first results. As you can see we repeated the experiment 5 times to get assure result precisions. From Table 7 we can see that the volume of gas produced constantly throughout.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work