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

To investigate the factors affecting the rate of reaction of calcium carbonate (limestone) with hydrochloric acid

Extracts from this document...

Introduction

SHURREEN MILES 10.G REACTION OF CALCIUM CARBONATE GCSE COURSEWORK AIM: To investigate the factors affecting the rate of reaction of calcium carbonate (limestone) with hydrochloric acid. SCIENTIFIC KNOWLEDGE: When you add hydrochloric acid to limestone it reacts giving off gases which is carbon dioxide, the concentration of the acid will also affect the rate of reaction like the surface of the limestone also if the water in the experiment is warm or cold. The scientific equation is CaCO3 (S) + 2HCl (aq) - CaCl2 (aq) + H2O (1) + CO2 (g). Example of the concentration is that when the concentration is in creased the particles will be closer together and when the solution is made warmer the particles move faster. PREDICTION: I predict that as the temperature of the acid increases, the rate of reaction will increase. ...read more.

Middle

2) Fill up beaker with 100mls of water, put the beaker on top of the gauze. 3) Heat the water up until it reaches 30C. 4) Pour 25mls of the 1.5 molar hydrochloric acid into the boiling tube. 5) Place the boiling tube in the beaker and put the thermometer in the boiling tube to make sure the acid is at 30C. 6) Fill the measuring cylinder up with water. 7) Turn the water bath, upside down over the cylinder and hold the bath down firmly. 8) Tip the bath and cylinder upside down, still holding them together firmly so that the bath is placed firmly on a flat surface with the cylinder inside it. Hold the cylinder tightly in the bath to make sure no water escapes. ...read more.

Conclusion

RESULTS: Temperature Test 1 Test 2 Test 3 Average rate of reaction 30 C 57ml/30secs 50ml/30secs 40ml/30secs 49ml/30secs 40 C 65ml/30secs 65ml/30secs 50ml/30secs 60ml/30secs 50 C 80ml/30secs 70ml/30secs 69ml/30secs 73ml/30secs 60C 100ml/30secs 97ml/30secs 91ml/30secs 96ml/30secs 70 C 130ml/30secs 127ml/30secs 99ml/30secs 119ml/30secs CONCLUSION: Like I said in my prediction as the temperature increased, so did the rate of reaction also as it says in my scientific knowledge the collision statement did take place. As the temperature became more the particles began to move faster which resulted in more collisions. EVALUATION: After evaluating my results they were not very useful, I repeated the method three times then I could find the difference between the results to work out the average, if I did this experiment again I think the equipment would have to be different. I could also change the amount of acid and limestone or even the temperature. ?? ?? ?? ?? ...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 Aqueous Chemistry 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 Aqueous Chemistry essays

  1. Marked by a teacher

    To investigate the effect of temperature on the rate of reaction

    4 star(s)

    28 150 94 92 95 94 71 73 72 72 57 58 56 57 30 31 35 32 160 98 97 98 98 81 82 81 81 63 64 62 63 31 34 37 34 170 100 100 100 100 84 85 84 84 69 71 71 70 35 36

  2. To investigate the rate of reaction between different concentrations of hydrochloric acid with metal ...

    Which I diluted, using a pre-set percentage, e.g. 20%acid-80% water. I reacted both of the reactants in the conical flask, and putting the stopper on it, where the carbon dioxide then travelled through the rubber tubing that was linking from the flask to the syringe.

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    used is equal to those used of Oxalic Acid (aq). Now that I know the mols present in the Oxalic Acid (aq) and the volume used in the titration I can work out the concentration of it. Moles = Concentration x Volume Concentration = Moles Volume Concentration = 0.0002882

  2. Investigate how the concentration of hydrochloric acid affects the rate of reaction between calcium ...

    can be decided. * Hydrochloric acid - To react with the calcium carbonate. * Bung - To allow the carbon dioxide gas to pass along to the gas burette. * Conical flask - Where the reaction between the marble chips and hydrochloric acid will take place.

  1. What Factors Affect the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate?

    Not all reactions happen as easily depending on the bonds of the atoms in each substance. If the bonds are strong a large amount of energy is needed for them to break, this is why substances with weak bonds will react spontaneously.

  2. To investigate the factors affecting the volume of carbon dioxide produced when a carbonate ...

    After choosing the factor that I will vary, I must take into account that all other key factors must stay constant. This is important, because then only do we know that it is the variable chosen that is affecting the volume of CO2 produced.

  1. The Factors Affecting the Volume of CO2 released when a Carbonate reacts with an ...

    So, in the procedure the constants with the highest volume of CO2 released will be used. Below are all the results for the preliminary work that took place. Finding Volume of Acid Using the following equations, it is possible for me to find out how much acid is needed to

  2. The factors affecting the volume of Carbon Dioxide gas produced when a carbonate reacts ...

    I will also expect to have graph with a straight line going through the origin. The graph that I should have is shown below: There are two forms of Calcium Carbonate that we could use. There was powder and chips.

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