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

Year 12 Chemistry Coursework: The Magnesium Statue

Extracts from this document...

Introduction

Year 12 Chemistry Coursework The Magnesium Statue Niall Boyle 12E Planning The Problem A statue, which is made of an alloy consisting mainly of magnesium, corrodes at different rates, at different times of the year. Background Knowledge There are some areas of knowledge that should be taken into consideration to help in devising an experiment to help determine the cause of the problem, and which gave me a greater understanding of the problem. A major factor in the decay of the statue is acid rain, which prevents the formation of the oxide coat that would normally form on magnesium preventing corrosion in air. Rain is naturally acidic, due to the CO2 dissolved in it, however when sulphur dioxide and oxides of nitrogen react with the rain water they form sulphuric, and nitric acids which make the rain strongly acidic. SO2 + 1/2O2 + H2O � H2SO4 It may also take the form of snow or fog. The sulphur dioxides and oxides of nitrogen come mainly from industry. Acid rain is currently a subject of great controversy because of widespread environmental damage for which it has been blamed, including eroding structures, injuring crops and forests, and threatening or depleting life in freshwater lakes. However the 1990 amendments to the Clean Air Act of 1967 put in place regulations to reduce the release of sulphur dioxide from power plants to 10 million tons per year by January 1, 2000. ...read more.

Middle

takenfor the magnesium to be entirely dissolved * Work out the average time taken for the magnesium to dissolve and record it * Repeat these steps mixtures:25cm3 acid + 5cm3 water 20cm3 acid + 10cm3 water 15cm3 acid + 15cm3 water 10cm3 acid + 20cm3 water 5cm3 acid + 25cm3 water * Record your results on graphs of time for reaction against concentration of acid and rate of reaction against concentration of acid Blank Table of Results Sulphuric Water Conc. Time 1 Time 2 Ave. Time Rate of Acid (cm3) (cm3) (mol/dm�) (s) (s) (s) Reaction (s �) 30 0 2.00 25 5 1.66 20 10 1.33 15 15 1.00 10 20 0.66 5 25 0.33 Predicted Graph Results Table of Results Sulphuric Water Conc. Time 1 Time 2 Ave. Time Rate of Acid (cm3) (cm3) (mol/dm�) (s) (s) (s) Reaction (s �) 30 0 2.00 19 19 19 0.053 25 5 1.66 20 25 22.5 0.044 20 10 1.33 31 29 30 0.033 15 15 1.00 77 55 33 0.015 10 20 0.66 89 63 76 0.013 5 25 0.33 175 201 188 0.005 Interpretation My first graph, time for reaction to occur against concentration of acid, shows a negative correlation, with the curve of best fit similar to 1/x, meaning that as the acid became more concentrated the faster the reactants reacted. ...read more.

Conclusion

The reason the rate of reaction increases with concentration is because the more concentrated a reactant is, the more particles there are that can take part in the reaction. This means there shall be a greater number of collisions per second between the reactants, and the more collisions there are the more often there shall be a successful collision, so the reactants will react faster. My results were fairly accurate with all but one point near the line of best fit on each graph. Since both graphs are really showing the same information it will only be necessary to work out the percentage of accuracy there is in my results. I will use the last point on the second graph as it is furthest from the line of best fit. The actual point was 0.044 for rate of reaction when it should have been nearer 0.039. So: (0.039/0.044)*100=Percentage of accuracy 0.886*100=88.6% As such I am 88.6% certain of my results. If I was doing the experiment again I would record three reactions for each concentration of acid to try and get a better average, and I would also use a burette to measure volume of water and sulphuric acid in each solution to improve the accuracy of my results. I would also increase the volume of acid used to 60ml and see if this causes the line of best fit on the second graph to be closer to the origin. ...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 Patterns of Behaviour 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 Patterns of Behaviour essays

  1. Marked by a teacher

    Rate of Reaction Chemistry Coursework

    4 star(s)

    At first we were getting a good set of results but then we couldn't see a pattern in our results. Most of our results were all over the place and we couldn't get any reliable results. After looking at our method and our results we realised that we had to change something to get a better set of results.

  2. What changes can be made to alter the amount of heat produced when magnesium ...

    What catalysts are doing when they make a chemical reaction go faster is to increase the chance of molecules colliding. The first method is by "adsorption"; the second method is by the formation of intermediate compounds. Adsorption This occurs when a molecule sticks onto the surface of a catalyst.

  1. To investigate the effect of the concentration of nitric acid on the rate of ...

    There are a number of reasons why these anomalies could have occurred, however. Firstly, because we had no means of regulating the temperature of the environment in which the investigations were conducted, the temperature would have affected the results in some way because temperature is one of the variables which

  2. The aim of the investigation is to examine the kinetics involved in the reactions ...

    a thermometer in the system (a thermometer consists of graduations of 1.0 oC). The effect of temperature in the experiment was an important element, which must be considered. This is because it may have influenced the rate in which an activated complex was reached.

  1. The purpose of this coursework is to investigate the factors which affect the rate ...

    The fastest reaction will therefore take place when the zinc is in fine powder form. c.) presence of catalyst The presence of a catalyst speeds up the reaction because a catalyst lowers the activation energy level required for the reaction to take place, the presence of a catalyst results in more successful collisions while the catalyst remains unchanged in form.

  2. Science Coursework

    Furthermore the temperature will be room temperature for all parts of the experiment and I will use the same volume of sodium Thiosulphate of an particular concentration. ? The main thing is that because I will investigate the affects of the concentration of sodium Thiosulphate solution on rate of

  1. Investigating the Effect of Different Concentration Of Acid Rain On The Rate Of Reaction ...

    Aim: The aim of this investigation is to investigate the effect of different concentrations of Sulphuric acid (H2SO4) on the rate of reaction between Sulphuric acid (H2SO4 ) Magnesium. Hypothesis: I predict that if I double the concentration of the Sulphuric acid (H2SO4)

  2. Enzyme Coursework.

    Method Apparatus: � two syringes � large beaker of water � conical flask � bung � delivery tube � syringe tube � 20 volume Hydrogen Peroxide solution � 20 volume yeast suspension solution � two small conical flasks � stop watch � 'V' shapes glass tube or oxygen output �

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