• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10

An investigation into the factors affecting the rate of reaction of indigestions tablets with acid.

Extracts from this document...


Chemistry Coursework, An investigation into the factors affecting the rate of reaction of indigestions tablets with acid. Planning, To start the investigation I thought about what affected rates of reaction. I managed to come up with 4 ideas: 1 Surface area 2 Temperature 3 Concentration 4 Mixing of the substances (stirring) I decided to do 2 different preliminary experiment so I could chose the best variable to investigate and see what equipment was necessary to provide us with an accurate set of data. Our first Preliminary experiment was testing what affect heat had on the rate of reaction. I planned a basic experiment, * I took a heatproof mat and placed a Bunsen burner on it. * I then put a tripod directly above the Bunsen burner on which I placed a conical flask with a bung and delivery tube tightly attached on. * I fed the delivery tube into a bowl of water. * Then a measuring cylinder was filled up with water, (to the very top of the cylinder) the cylinder was then turned upside down whilst a hand was placed over the open hole of the cylinder with pressure letting no water out. It was the placed under the water in the bowl (hole first). * I removed the hand that was covering the hole of the tube when it was under the water of the bowl. The water remains inside the cylinder all the way to the top, this will allow us to see how much gas is given off by the amount of water forced out of the tube. * The delivery tube was then placed inside of measuring cylinder (to collect any gas given off). * A timer was needed to time how long the experiment took. * The Conical flask was then filled up with 100cm3 of acid; this was then heated to the desired temperature (of which there was 5). ...read more.


Method, For the real experiment I decided to collect the gas given off up to 70ml, although our preliminary results didn't reach 70ml given off I knew that when the experiment was done accurately with the right amounts of the substance (100 ml of acid and a full tablet) all of the results would be able to reach 70ml (I also knew this as others using full tablets were all getting in excess of 70ml). In the preliminary experiment only half tablets were used and only 50 ml of the acid were added which may not have produced all the gas required to reach 70ml although the tablet had dissolved indicating all tablet was used up. I changed it so 100 ml of acid were added not 50ml and a whole tablet was used this meant the variable of surface area can be kept constant through out the experiment as cutting may result in either 2 lumps of tablet being used as a half. Or simply the cut may go in a different angle revealing more tablet area to the acid. Also through the preliminary experiment I discovered that a measuring cylinder was not very accurate as the markings are not as accurate as the burette. I therefore, used a burette for both water and acid in the experiments to create the concentrations. * Take a burette and fill it up with acid, make sure it fills up to the zero (if not drain until at zero), otherwise extra or not enough acid may be filled into the beaker. * Measure 5 different amounts of acid into 5 separate beakers (20ml, 30ml, 40ml, 50ml and 60ml) by slowly letting the acid go drain into the beaker from the burette (stopping the acid when it reaches the desired amount released). These concentrations were used in the preliminary experiment and provided a good range of results (a quite low concentration - 20% and a reasonably high concentration - 60%). ...read more.


This down through human error, there is no way you will be able to say for example stop the stopwatch as soon as the reaction has finished because the signs I look for a quite inaccurate - observe the stopping of carbon dioxide being release and the tablet no longer being visible therefore, to use split seconds for times accuracy would be ridiculous. I am pleased with my method and believe that it was definitely sufficient to obtain the evidence I needed to prove my prediction right. It allowed me to make concentrations that were of a good accuracy that is essential to this investigation. The reliability of my results I would say is extremely good; when I compare all 3 graphs I can see that the gradient for each one is basically exactly the same. The quality of the real experiment and the repeats was I think, very good, I can see that in both experiments they reached almost exactly the same rate for each point (even the preliminary results show good correlation with the 2). A variable that affects quite a lot was not considered enough during my experiments. I can see that from my very first preliminary test (on temperature) that temperature is very significant to the rate of reaction. Although I completed each experiment on the same day (1st experiment one day repeats another) at the same time the temperature may have varied per concentration due to a sudden change in temperature. However this would probably not have been enough to affect our results considerably but taking the temperature before each concentration test would have been good as it might have explained so anomalous results or at least may show you if the temperature has an affect on the rate when it is varied within a few degrees. So in conclusion if I were to extend my investigation I would use a thermometer to measure the temperature in future before the reaction takes place and I would also vary the temperatures from 50% to 90% at 5% intervals to see what happens around this area in more detail. ...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)

    Equipment List: * Calcium carbonate (medium chips) - the solid reactant * Hydrochloric acid - the liquid reactant * Spatula - to measure out accurate amounts of marble * Measuring cylinder - to accurately measure the 30ml of hydrochloric acid * Ice - to make the temperature fall accordingly for

  2. To investigate three factors that affect the rate of cooling a liquid and to ...

    Conductors If the container storing the water is made of a heat conductor, the water or other liquid would cool more quickly, as heat energy is being lost all the time, transferring from the water to the container. A heat conductor is any material that offers little resistance to the flow of heat energy.

  1. Indigestion Tablets Investigation

    The higher the temperature the shorter the time it takes for the tablet to completely react with the acid. This is because, according to collision theory, molecules with more energy will move about quicker and therefore the particles are more likely to collide so the reaction will occur more quickly.

  2. Planning an Investigation To Determine The Effectiveness of Indigestion Tablets at Neutralising Excess Stomach ...

    Too much calcium can damage the kidney and lead to calcium deposits. CaCO3 + HCl ----------> CaCl + H2O + CO2 Magnesium Hydroxide: This forms magnesium chloride (a harmless salt) and water in the stomach to calm indigestion. Mg(OH)2 + 2HCl ----------> MgCl2 + 2H20 EQUIPMENT: 1 burette, 1 clamp

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

    (aq) turned the solution a deeper shade of purple. Also the colour faded very quickly after the Potassium Manganate (VII) (aq) had been added. Even after the end-point had been reached (i.e. the solution remained coloured for 30 seconds) the colour continued to fade so that there was nothing to compare the solutions colour too, to help with determining the end point of the reaction.

  2. To see which antacid tablet is the most efficient out of 4 samples.

    The only exception to this is the antacid tablet; they have to vary otherwise there wouldn't be an experiment. If this is all followed then a fair test should happen. Key Factors/ Variables- The only variable in this test are the antacid tablet, of which I must change once I have a consistent set of results for the tablet before.

  1. Collision Theory

    will reach the top of the activation energy to form products also doubles thus doubling the rate of reaction. In other words: Rate (is proportional to) Concentration. Two graphs will be drawn in this experiment, a time-concentration graph and a rate-concentration graph.

  2. Aspirin Investigation

    Complete the crystallization by further cooling the mixture in an ice-water bath. Collect the crystals on a Buchner funnel by suction filtration, wash them with a little cold water and press them firmly with a rolled cork or glass funnel to remove as much water as possible.

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