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

Investigation on how the rate of reaction changes as the concentration of an acid changes

Extracts from this document...

Introduction

Chemistry Coursework 01 May 2007 Alex Hall (J) Investigation on how the rate of reaction changes as the concentration of an acid changes Skill P : Planning The investigation that we are studying in this piece of Coursework, is how the rate of the reaction between Magnesium and Hydrochloric Acid changes, as the concentration of the Acid is decreased. The equation for this investigation is as follows: Mg (s) + 2HCl (aq) MgCl2 (aq) + H2 (g) I predict that as the concentration of the acid decreases, the rate of reaction will also decrease. Collision Theory says that the more concentrated the reactants, the more collisions will occur. This also explains why the reaction is quickest at the start; it is because the reactants are in their most concentrated state. As the reaction progresses, the concentration of the reactants decreases, and therefore so does the rate of the reaction. In order for the reaction to take place, the particles must collide; and secondly, the smallest amount of energy, the activation energy must be reached. If the activation energy is very high, then there will be a small number of particles able to react, and therefore the reaction rate will be slower. ...read more.

Middle

I am going to keep the length of the magnesium at a fixed length of 5cm. From my preliminary work, I can see that the yield of 5cm of magnesium, when reacted with hydrochloric acid, is enough to give me clear results when I come to plot the graphs. * The third and final variable is whether or not I use a catalyst to speed up, or slow down my reaction. A catalyst is a chemical which speeds up (or slows down) a chemical reaction. A positive catalyst lowers the amount of activation energy required, so the reaction happens faster, the catalyst is not 'used-up' during the reaction. For this particular investigation, I am not going to use a catalyst. As I have mentioned earlier, I am going to change the concentration of the acid, by adding water. I will need to make sure that I measure the amount of acid and water correctly. When I add some water to the acid, I will need to be certain that the two liquids are evenly mixed together in the test tube, I will do this by shaking the test tube. ...read more.

Conclusion

* 20 cm� acid + 30 cm� water * 20 cm� acid + 40 cm� water * 20 cm� acid + 50 cm� water The reason behind repeating the experiments is so that if in the first experiment for the lowest concentration, the magnesium is dirty; it may not produce accurate results. So in the next section, I am going to display my tables with the original and repeat experiment, and the averaged result. The graphs in the analysis will make use of the average results. There are a few safety measures that I must take, when conducting this investigation. * We must wear our safety goggles and lab coats. * Hydrochloric Acid may burn clothes and skin if it comes into contact with them. * When the two chemicals are mixed, an impurity may cause a small explosion, so if we are wearing our safety goggles, the chance of anything getting into our eyes is greatly reduced. * Most chemicals are dangerous if swallowed, therefore we must not taste any of the products or reactants, and we must also not put a pen or any other item into our mouths because they may have been in contact with one of the chemicals. ...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. Aspirin Investigation

    In the second tube, add 5 drops of pyridine. In the third and fourth test tubes add 5 drops of boron trifluoro-etherate and 5 drops of concentrated sulphuric acid, respectively. Put all the tubes in a beaker of hot water for 5 minutes to dissolve solid material and complete the reactions, and then pour all the solutions into a

  2. Antacid Investigation.

    Predicted volume of acid = 0.01 moles divided by 1= 0.01 dm cubed 0.01 x 1000 = 10 cm cubed to neutralise the antacid. Calculations for Rennie (pepper mint flavour) antacid tablet. Note: This tablet is different to the ones above it has an extra carbonate ingredient so it will be different.

  1. Free essay

    Chemistry investigation

    Here is a labelled diagram of what the experiment looked like: Results: Time (seconds) Result 1 (ml2) Result 2 (ml2) Result 3 (ml2) 10 20 30 40 50 60 Evaluation of Preliminary Methods Each of the experiments above has limitations that strongly influenced the results.

  2. whether the strength of Hydrochloric acid will affect the speed of the rate of ...

    175 50 68 64 0.2 cm�/sec 0.2 cm�/sec 0.2 cm�/sec 180 51 70 65 0.2 cm�/sec 0.4 cm�/sec 0.2 cm�/sec 185 52 72 67 0.2 cm�/sec 0.4 cm�/sec 0.4 cm�/sec 190 53 73 68 0.2 cm�/sec 0.2 cm�/sec 0.2 cm�/sec 195 54 75 69 0.2 cm�/sec 0.4 cm�/sec 0.2 cm�/sec

  1. Reactivity Series Investigation

    Never give anything by mouth to an unconscious person. Get medical attention immediately.If there is skin contact with calcium powder Wipe off excess material from skin then immediately flush skin with plenty of water for at least 15 minutes. Remove contaminated clothing and shoes. Get medical attention. Wash clothing before reuse.

  2. Rates of Reaction

    product in a particular reaction is intuitively defined as how fast a reaction takes place. There are numerous ways a reaction can be influenced by certain factors of which some are listed and explained further below: Concentration Reaction rate increases with concentration, as described by the rate law (the rate

  1. What effects the rate of a reaction

    So simply I predict that as the concentration of the solution increases, the faster(shorter) the rate of reaction will be. So as the molarity of the concentrations increases the shorter the length will be for the magnesium to dissolve. I believe this because increasing the concentration of the reactants increases

  2. Rate of Reaction

    The reacting molecules however have to overcome the activation energy to react and if the activation energy is high then only the most energetic molecules will be able to overcome it making the reaction slower. If, however, the activation energy is small then more of the collisions will be effective and the reaction will be faster.

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