• 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...

Introduction

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.

Middle

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.

Conclusion

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)

    Some reactions are very fast, e.g (the formation of silver chloride precipitate when silver nitrate and hydrochloric acid solutions are mixed.In this investigation we will test different concentrations of acid reacting with magnesium. HYPOTHESES A reaction occurs when particles collide.

  2. Marked by a teacher

    Rate of Reaction Chemistry Coursework

    4 star(s)

    fast and we didn't have time to get a good set of results as it had all reacted after 20 seconds. After we tried to do the same but instead of using 10ml we used 5ml of hydrochloric acid. We also decided to only use 0.2 grams of magnesium.

  1. Marked by a teacher

    Lab report rates of reaction

    3 star(s)

    reacted with the three different acids( Hydrochloric acid, Nitric Acid and Sulphuric Acid), over a constant time of 3 mins. The volume of the Co2 will then tell us how the differentiation in the size of the Calcium carbonate pieces has affected the overall rate of reaction.

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

    Then I will follow my finger from the line, horizontally, to the "y" axis, and see what the approximate volume of the Gas Jar is. Results TIME CANDLE IS LIT FOR (s) Volume of Glass Beaker (cm 3) Test 1 Test 2 Test 3 AVERAGE 105 7.66 5.6 7.92 7.06

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

    increase - some would be moving extremely quickly whilst others extremely slowly. Therefore, as temperature increased, more hydrogen peroxide particles would have the activation energy required for a reaction to occur, and so temperature increases, so does rate of reaction.

  2. An Investigation of the Effect of Copper Sulphate on Catalase Activity.

    * The fifth contains 0ml of copper sulphate solution and 20ml of water to create a solution with a copper sulphate concentration that is 0% of the first or a 0mol copper sulphate concentration. Lastly, to test whether or not copper sulphate acts as a reversible inhibitor, add five 1cm3

  1. Investigating the reaction between zinc and copper sulphate

    Some heat might have escaped from the open cup. There could have been errors in the reading. The stirring could not have been thorough and consistent. These results can be further improved by: Using a more insulating lid to prevent heat loss.

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

    CaCo3 (s) + 2HCL(aq) ---> CaCl2(aq) + H20(l) + CO2(g) Salt produced - Calcium carbonate Acid used to neutralize the reaction - Hydrochloric acid This equation tells me the reactants needed and the products produced but doesn't explain how much is needed to for an accurate reaction to take place.

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