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

The Reaction.

Extracts from this document...

Introduction

The Reaction The word equation for this reaction is: Copper Sulphate + Iron --> Iron Sulphate + Copper The balanced chemical equation for this reaction is: CuSO4(aq) + Fe(s) --> FeSO4(aq) + Cu(s) This reaction falls under several categories of chemical reaction, namely: * Displacement reaction * Exothermic reaction * Redox reaction I will now explain each of these reactions in detail. Displacement Reaction In a displacement reaction, the more reactive substance in the reaction takes the place of the less reactive substance. As can be seen from the equations written above, the iron takes the place of the copper in the copper sulphate solution. The reaction can therefore be classed as a displacement reaction. Redox Reaction 'Redox' stands for REDuction / OXidation, meaning that in the reaction, there is one substance which gains oxygen and another which loses it. Reduction and oxidation always happen together - if one thing is reduced, another is oxidised. By looking at the equations, it is easy to see that iron has been oxidised - gained oxygen, while copper has been reduced - lost oxygen, by losing the sulphate, SO4, to the iron. However, it is also possible to tell which substance has been reduced and which has been oxidised by looking at how the charges of the substances change in the equation. ...read more.

Middle

I could now proceed with my investigation. Apparatus Anhydrous copper (II) sulphate - with which to make the solution for the experiment Distilled water - to dissolve the copper sulphate to make solution Fine iron filings - to put into the solution to carry out investigation Electronic weighing scales - in order to weigh out iron and copper sulphate quantities fairly accurately Boiling Tubes - in which to place solution and iron Measuring cylinders - to measure out quantities of distilled water and copper sulphate solution Thermometer - to record highest temperatures reached because of the exothermic reaction Stirring rod - to stir the copper sulphate while making solution Bunsen burner - to help the copper sulphate dissolve into the distilled water Hypothesis I predict that as the concentration of the copper sulphate solution gets weaker, the amount of energy released will decrease proportionately, i.e., if there is a change of 10 degrees Celsius when the iron is in a 0.8 M solution, there will be a change of 5 degrees Celsius in a 0.4 solution. However, if the concentration of solution was more than 1 mole, there should be no additional temperature rise; the ratio of 1M of solution to 1M of iron would produce the maximum temperature rise. ...read more.

Conclusion

Therefore, it is likely that most of the iron did react. However, during this reaction, a layer of copper will have formed over each iron filing. This would mean that the inside of each grain of iron would not have been able to react with the copper sulphate. Therefore, in effect, less than one mole of iron was added to the copper sulphate because not all of it was able to react. This resulted in lower temperature increase than expected. It would have been very hard to solve this problem as I would have had to work out how much a mole of iron was, taking into account the size of each iron filing as this would determine the size of the copper layer surrounding it. The best I could have done was to use even finer iron filings; however, I would still have had the same problem although to a lesser extent. 3) As explained above, the iron filings had a very large surface area because of their minute size. Since iron is a fairly reactive metal, it would have reacted with oxygen while in storage, resulting in a layer of iron oxide covering it. Therefore, when I weighed out a mole of iron for my experiment, I was weighing out both iron and iron oxide. This problem could have been reduced by storing the iron very carefully so that it should come into contact with the least amount of oxygen possible. ...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. Synthesis of Iron (II) Sulphate FeSO4

    For about 1 day later, we will find out some nice formed crystals appear at the bottom of the bottle Advantages

  2. Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress ...

    By mixing the solution as it is made, it means that the solutions will not have all the copper sulphate at the top or bottom, the whole thing will diffuse quicker. This batch can be used as a control as it has no copper sulphate in it.

  1. Determining the purity of Iron Wool.

    x 100 = 90.9% CONCLUSION The aim of this experiment was to see how many molecules of water of cryatallisation were in a sample of sodium carbonate crystal. Once sample was added to the ionized water it readily dissolved without a change in environment i.e.

  2. Rates of Reaction

    that the slope of the of the reaction curve decreases with time, this is due to all reactant particles being used up and the successful collisions have reached their optimum, I would expect to see such correlation within my graph.

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

    In most redox reactions an indicator needs to be added to the experiment to show the end point of the reaction but this is not necessary as the reaction that occurs produces a very obvious colour change (7). The Fe2+ ion present in the Iron (II)

  2. To organise 5 given metals into a reactivity series using 0.2 M Copper (II) ...

    Moles in solution = molarity x volume of solution Moles of CuS04=x 20 = 4 x10-3 moles of CuS04 in 20cm3 of 0.2 molar solution. Since we now know how many moles of Copper Sulphate we have, and since we know the reacting ratios are 1:1, we now know that

  1. Investigation to determine the lowest concentration of copper (II) sulphate solution that brings full ...

    sulphate solution needed to conduct the experiment. The reason for adding water is to dilute the copper (II) sulphate solution. Test tube A has the solution at full concentration this concentration is decreased in test tubes A through to F as more and more water is added.

  2. Rate of Reaction

    When we increase the concentration, we are increasing the frequency of collisions between the particles. However changing the concentration does not change the speed at which the particles are moving. A good way of describing this is For example if you are in a 60,000 capacity football ground and there

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