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

Metal Reactivity Coursework

Extracts from this document...


Metal Reactivity Coursework Aim: To put the following metals into a reactivity series: Magnesium (Mg) Zinc (Zn) Iron (Fe) Calcium (Ca) Copper (Cu) Aluminium (Al) Method Plans: 1) Secondary Source: "Chemistry Counts" by Graham Hill. Record visual reactions, i.e. how bright the reaction is, how violently it reacts, and how fast the reaction is completed. This, however would be impossible with the metals concerned as, not only is it highly inaccurate but also slow: Iron takes a long time to react. The other reason is that you would then need a scale of violence for comparison of the various metals. 2) Record the amount of hydrogen produced upon reacting each metal with hydrochloric acid over a constant period of time. The higher the rate of hydrogen produced, the more reactive metal. Unfortunately the amount of hydrogen produced in each case is negligible. To get enough hydrogen produced to give meaningful results, large amounts of acid and metal are required. According to another secondary source, 30g of hydrochloric acid reacting with 0.54g of Aluminium gives of 0.067% of that- 0.02g as hydrogen. You would need at least ten times that much to be able to obtain a recording, therefore the experiment is not possible. 3) Measure the enthalpy change of reaction by measuring the heat produced at set intervals, thereby building a graph to extrapolate a curve giving us a maximum temperature rise. ...read more.


hydrochloric acid at a concentration of 2mol/dm3 mercury thermometer graduated to 1�c electronic timer plastic lid Two lots of 0.1 mol of each metal: Table of amount of each metal needed: Metal Mass of 0.1 mol (in g) Calcium 4 Magnesium 2.4 Aluminium 2.7 Zinc 6.54 Iron 5.6 Copper 6.35 A degree of accuracy is important, which is why everything used in this experiment should be constant except for the metal involved. Testing each metal twice makes sure an accurate reading is taken, without fear of using a 'bad' result. Diagram of apparatus: Key factors: Room temperature. Room pressure. Key Variables: Concentration of acid- must be constant. Amount of acid- a constant volume (0.1 moles).( The reason for only 0.1 mol is that you need two moles of HCl to react with one mole of a metal. So as I want to have an excess of metal I am only going to use half of the acid needed to react with the metal) Mass of metal- 0.1 mol Time readings are taken every 30 seconds for nine and a half minutes Having the above as constants adds to the accuracy of the experiments. Amount of acid needed. I want to use double the amount of metal than acid needed to react with the metal. The chemical equations are the following: (I am using M as the symbol for metal, and assuming M forms M�+ ions we can write a general equation as) ...read more.


If I was to do the experiment again and I wanted as accreat results as i possibly could and the experiment to be as fair as it could, I would have to use an more accreat way of measuring the temperature rise such as an sensor to a computer, as when I did it I only had an thermometer in if I wanted it to go down to the decimal placing had to be gess work as it was in this experiment. I would also change the way I insulated the experiment, not that mine was not effective but there are even better ways of insulating it. I would also use metals that had not been exposed to the air as the air reacts with them and on some metals such as iron it forms an less reactive coat on the metals. That is what I believe happen to all of my meals apart from Magnesium, as there paths should have followed that of Magnesium in the sense that it goes up then down, but in my experiment they did not, this I believe is because the had all ready reacted with the air forming an coat on the metals and that is why I took longer for them to react as the acid had to react with these coat first. Rhys Beddoe i ...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

    chemistry coursework

    4 star(s)

    Stir the solution until it turns a blue/black colour and the cross underneath is not visible. 28. Record the time taken. 29. Wash your apparatus. 30. Pour 10 cm� of potassium iodide, 40 cm� of sulphuric acid and 5 cm� of special indicator into the 100 cm� measuring cylinder.

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

    The solutions were keep in the water baths or ice buckets before and during experiments so that the solution remained at a constant temperature. As the volume of Sulphuric Acid (aq) added to the Iron (II) Ammonium Sulphate (aq) had to be in excess to supply H+ ions I felt


    All theses steps should ensure that reliable Precision and Accuracy: * The balance is a precision instrument with an accuracy of 0.01 grams. This is sufficient for the task at hand. * The syringe is accurate to 1cm3, however it can be seen when the syringe marker is halfway through

  2. metal extraction and reactivity

    Extraction of metals from their ores. * Ores are: carbonates, oxides or sulphides of the metal mixed with impurities. * Large lumps of the common ores are first crushed and ground up by very heavy machinery. * Some ores are already concentrated.

  1. Free essay

    Chemistry Coursework

    * Wire mesh - to stand the beaker on * Heat proof mat - to protect the table from the heat of the Bunsen burner * Thermometer - to measure the temperature. * Stop clock - to time how long the reaction takes.

  2. Neutralisation Coursework

    But as this is past the point of neutralisation she took 0.2ml off the reading to get the exact result. In the preliminary experiment it proved that it takes approximately the same amount of Acid to neutralise 20ml of a base.

  1. Investigating the kinetics involved in the reaction of metals with acids.

    Using concentration greater that 3M will cause a reaction to occur too quickly. This will make timing inaccurate and provide unreliable results. Gas & Acid Volumes - I am using 2.5cm strips of magnesium for each reaction, which weighs 0.025g.

  2. Investigate 'How much gas is released when a metal reacts with an acid.'

    the beaker into it I will have to make sure that the Magnesium doesn't touch the Sulphuric Acid as if it does the reaction will occur. After this I will shut the beaker with a rubber bung that has a delivery tube in it and I will place the other

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