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

Rates of Reaction Practial

Extracts from this document...


Rates of Reaction Practical Aim: The aim of this investigation is to investigate how the rate of reaction of Calcium Carbonate (CaCO3) with Hydrochloric acid (HCl) could be affected by surface area. Equation: HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l) Hypothesis: I predict that the more the surface area the faster the rate of reaction because it increases the chances of collision. This is because more calcium carbonate is exposed to the acid molecules so they are more likely to collide. When measured in the same mass the smaller chips have a larger surface area altogether. Here is a diagram to show this: (if cut into 8 equal pieces) ==> Apparatus: - Two beakers (400ml) - Large Calcium Carbonate Chips (5g) - Small Calcium Carbonate Chips (5g) - Calcium Carbonate Powder (5g) - Hydrochloric Acid 1M (100ml) - Spatula - Accurate Scale - Stopwatch Method: 1. ...read more.


0.011g 0.073g 0.291g 90 0.025g 0.087g 0.298g Results Graph: Conclusion: From observing my results I have found out that powder has the quickest rate of reaction, then comes small marble chips and lastly large marble chips have the slowest rate. This is because when the size of particles is reduced it increases the surface area available for collisions to occur. When the chip is larger the acid particles can only collide with the edge of the chip. If the chip is cut into several smaller pieces, the acid particles (in the second diagram) can now reach the centre part of the original larger chip. This is why the powder had the quickest rate of reaction. In conclusion my prediction was right. I predicted that the smaller the chips the faster the rate. Evaluation: When I started the experiment my original plan was to react zinc with hydrochloric acid. ...read more.


This means that I could only compare and assume that the powder had more surface area than the large calcium carbonate chips. I then figured out a way to solve this problem, which is to purchase calcium carbonate chips cut into cube form in different sizes. This way I would be able to measure and calculate the surface area of each size of calcium carbonate cube therefore I would actually know the surface area. This way not only would I have more surface areas to confirm the trend, my results would be much more accurate and clear. If I could do this experiment again I would repeat my method but record every 30 seconds instead so that the change is more visible, and record until 3 minutes so that the calcium carbonate would dissolve more thoroughly. I would also repeat it several times to make sure my results are accurate and reliable and that my prediction was right and experiment on more surface areas to confirm the trend. ?? ?? ?? ?? ...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 Classics section.

Found what you're looking for?

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

Here's what a teacher thought of this essay

3 star(s)

The report is fairly straight forward. The experiment is of limited complexity and requires a limited degree of precision. The data collected is of a reasonable quality. However the lack of repeats limits the reliability. There are improvements suggested throughout.

Marked by teacher Cornelia Bruce 18/04/2013

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 Classics essays

  1. Marked by a teacher

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    The rate of a chemical reaction is a measure of how fast the reaction takes place. It is important to remember that a rapid reaction is completed in a short period of time.

  2. Investigation on how long a candle burns under a glass beaker.

    282 22 24.4 23.5 23.3 500 36 32.6 40 36.2 1100 93.2 60 84 79.1 600 32.4 30 27.4 30 GAS JAR 11.6 14.6 17.3 14.5 Analysis From my results I have found out the Gas Jar has an approximate volume of 200 cm cubed.

  1. Factors Affecting the Rate of Catalytic Decomposition of Hydrogen Peroxide.

    Mass Lost (g) Mass Lost (g) Mass Lost (g) 5 0.14 0.16 0.13 0.14 10 0.19 0.21 0.22 0.21 15 0.26 0.27 0.29 0.28 20 0.34 0.34 0.36 0.35 25 0.39 0.46 0.42 0.41 30 0.49 0.58 0.49 0.49 35 0.53 0.66 0.56 0.55 40 0.61 0.68 0.60 0.61 45 0.63 0.69 0.63 0.63 50 0.64 0.69 0.63 0.64

  2. A-Level Investigation - Rates of Reaction – The Iodine Clock

    - 298K and 1 ATM pressure. For example; When varying the volume of Hydrogen Peroxide in the mixture it will be the independent variable, the controlled variables will be the volumes of the Thiosulphate, Potassium Iodide and Sulphuric Acid. The overall volume will be kept constant by the addition of a measured volume of distilled water

  1. Determining the Enthalpy Change of the Decomposition of Calcium Carbonate.

    Evaluation The enthalpy change for the reaction CaCO3 (s) heat CaO (s) + CO2 (g) Should have been +178 Kj mol -1 , this figure was according to the text book 'understanding chemistry for advanced level ' Errors must have occurred in the experiment because my result for the (H3 was over 100 Kj mol -1 out.

  2. Investigating the reaction between zinc and copper sulphate

    does not rise as high as 1.01, 0.91 or 0.81 grams of zinc. I also predicted that the mass of zinc would rise in direct proportion to the temperature. We can see that this prediction is not true as then you would expect the temperature to almost double from 0.41

  1. The Iodine Clock Investigation

    time will have a half-life that isn't constant, but one that increases dramatically as the reaction proceeds. This graph is visibly much 'deeper' than a graph showing a first order reaction. N.B. The graphs above only show the order of a reaction with respect to substance A, and do not necessarily show the overall order of the reaction.

  2. The Effect of Catalase in the Breakdown of Hydrogen Peroxide

    This includes water poured into the burette to the water that will be used throughout the whole experiment in the water bath. This is so that the experiment can have results that are fair and are not manipulated by the water temperature.

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