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

Surface area vs Rate of Reaction

Extracts from this document...


The Effect of the Particle Size on the Rate of Reaction CaCO3 (s) + 2HCl(aq) --> H2O (l) + CO2 (g) + CaCl(aq) Variables: Variable Methods of Measurement Independent Size and Surface area of the CaCO3 particle; in chip of approximately 3x3x3 mm in size or in powder form. Pre-measured. Materials are given. Dependent Volume of gas produced in 3 minutes measured by the graduated glass collecting tube Using a graduated glass collecting tube. The gas produced will push the water out of the tube and the volume of gas can be read on the tube Controlled Variables: Variables Why it must be controlled? How could it impact the results? How it will be controlled Condition of where the CaCO3 and HCl are kept Different conditions of the CaCO3 will result in different inaccurate measurement when the experiment is carry out, some CaCO3 might have been kept at different temperature, which would alter the amount of energy they have, thus changing their collision potential with HCl molecules Both the powder and the chip CaCO3 and HCl solution must be kept in the same condition and temperature to ensure that throughout the experiment, they have consistent energy and collision potential Molarity of HCl This different amount of HCl liquid will cause the glass production to varies if were to used the different volume of HCl Use 8ml of 2M HCl in every ...read more.


CO2 produced from the reaction between 0.6 g of CaCO3 powder and 8 ml of 2M HCl over 3 trials and the mean, in intervals of every 10 seconds. The uncertainty is 0.05 ml as the readings are analog and the smallest unit is 0.1 ml Time/s Volume of CO2 produced /ml (�0.05) Volume of CO2 produced /ml (�0.05) Trial 1 /ml (�0.05) Trial 1 /ml (�0.05) Trial 1 /ml (�0.05) 0 0.0 0.0 0.0 0.0 10 22.0 17.0 12.0 17.0 20 32.0 17.0 21.5 23.5 30 35.0 35.0 27.0 32.3 40 39.0 42.0 31.5 37.5 50 41.0 43.0 34.5 39.5 60 42.0 44.0 37.0 41.0 70 43.0 45.0 39.5 42.5 80 43.0 46.0 41.5 43.5 90 44.0 47.0 44.5 45.2 100 44.0 47.0 46.5 45.8 110 45.0 47.0 48.0 46.7 120 46.0 47.0 49.5 47.5 130 46.0 47.0 49.5 47.5 140 46.0 48.0 49.5 47.8 150 46.0 48.0 49.5 47.8 160 46.0 48.0 49.5 47.8 170 46.0 48.0 50.0 48.0 180 46.0 49.0 50.0 48.3 Analysis Figure 1: Amount of CO2 released from the reaction between HCl and CaCO3 Powder-a scatter graph of raw data collected over 3 trials showing volume of CO2 as the independent variable and how it changes over a period of 180 second. Error Bars represent uncertainty(�0.05 mL) ...read more.


The CO2 gas needed to build up enough pressure to overcome the water in order to go through. This causes the gas to travel inconsistently, and making the result inconsistent as well. This could be solved by changing the direction of the tube and using a shorter tube. Another cause for loss of gas is the inability to capture the gas immediately as the reaction starts. As soon as HCl is poured into the flask with CaCO3, the reaction starts and produces CO2, water, and CaCl, however, the flask has to be opened in order to transfer the solution, and some gas may be lost in that opening. This is very important as the beginning section is where the rate of reaction is the greatest. This can be solved by using teabags or other similar methods to separate the reactants without exposing them to the environment. Another major error in the experiment is the size of the CaCO3 chips. As mentioned in the qualitative observation, some marble chips are larger than others, causing that trial to have less surface area while having the same mass. As discussed above, this could potentially cause the reaction to be much slower due to less collision. This can be solved by using a large chips that we can cut by ourselves so that we can control the size, surface area, and volume of the reactants ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate 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 International Baccalaureate Chemistry essays

  1. Experiment to observe how rate of reaction depends on the surface area.

    * We put the powder in the beaker. * We time the reaction and the temperature. V) The table of results: Size of the particles Time of the reaction Observations A quarter of frizzy tablet in one piece 40 seconds When we put the quarter of tablet in the baker the reaction makes a fizz and some bubbles during 40s.

  2. Design Lab, HCl + Marble chips

    > Temperature (�C)- If you increase the temperature of a reaction, it will speed up and so the test will not be fair. Hence, the temperature of both the reactants will be that of the room temperature. > Time for the reaction.

  1. FInding the percentage purity of CACO3 in egg shell

    7. Phenolphthalein indicator 8. Burette 50cm3 (±0.02 cm3) 9. Volumetric flask 250cm3 (±0.12 cm3) 10. 7 conical flask 250cm3 11. Dropping pipette 12. Stirrer 13. Stirring bar 14. Stirring rod 15. Glass funnel 16. Plastic funnel 17. Distilled water Procedure 1. Take the egg shell and make sure it’s completely dry 2.

  2. Calculate % of caco3 in white egg shell

    A point will be reached when the solution will become completely pink and the shaking of the conical flask will not dissipate the colour.

  1. Reaction Rate

    so that evidence of the experiment and setup can be visually shown. 1. Place the plastic, ice-cream container on the desk adjacent to the retort stand and fill it 2/3 of the way up with water from the tap. 1.

  2. Design -How does the surface area of Calcium carbonate (CaCO3) affect the rate of ...

    solution * 10 g of calcium carbonate (CaCO3) Safety Materials * Gloves * Safety glasses Diagram Procedure 1. Safety glasses and gloves were worn. 2. Known mass (10 g) of calcium carbonate granules was placed in a flask and the apparatus was set up as shown, with the plunger of

  1. Experiment Plan. Effect of Surface Area on Rate of Reaction

    Since the concentration of HCl(aq) and mass of CaCO3 are constant, the volume of CO2 produced is constant. However, the more finely divided a solid is, the larger is its surface area. According to the collision theory, the rate of a reaction is directly proportional to the number of effective collisions per second between the reactant molecules.

  2. Investigating the Effects of Surface Area on the Rate of Reaction

    Magnesium ribbon 2. Hydrogen Gas will be the gas collected 1. 3 Trials will take place 1. Mass of Magnesium ribbon in: 1. Trial 1: 0.064 grams 2. Trial 2: 0.063 grams 3. Trial 3: 0.065 grams CaCO3 + 2HCl ? CaCl2 + H2O + CO2 1. Marble Chips 2.

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