• 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...

Introduction

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.

Middle

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.

Conclusion

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)

    Record the time. 35. Record all your results in a table and repeat the experiment. NOTE: Potassium iodide, sulphuric acid and special indicator containing starch can be mixed, i.e. in the same measuring cylinder. Hydrogen peroxide and water can also be mixed together.

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

    being used in the reaction first to 10 cm3 and then to 5 cm3 as I realised that 10 cm3 was still taking too much Potassium Manganate (VII) (aq) to reach the end point of the reaction. I also found that the temperatures of the solutions under test were changing once the Potassium Manganate (VII)

  1. DECOMPOSITON OF HYDROGEN PEROXIDE WITH HEAVY METAL CATALYSTS

    * An overall should be worn when handling hydrogen peroxide. * Goggles should be worn when adding the oxide to the peroxide, although they are not needed throughout the rest of the experiment. Reliability of Results: * When collecting the gas, the attachment of the rubber bung should be very quick to minimise any loss of gas.

  2. My aim is to put zinc, iron, magnesium, nickel and calcium into an order ...

    Nickel will hardly react. Method * The things that will change in the experiment are the temperature * I will carry out the experiment by putting the metal powder in a test tube and then mixing with it hydrochloric acid and I will measure the temperature every 30 seconds for five minutes.

  1. metal extraction and reactivity

    Hydroxides of this type are said to be amphoteric. * Also the oxides of such metals are amphoteric as they react with both acids and alkalis. e. Discovery of metals * An ore is a naturally occurring mineral from which metal can be extracted. * Metals which are highly reactive are difficult to isolate.

  2. Free essay

    Chemistry Coursework

    * Measuring cylinder - to measure the volume of hydrochloric acid. The chemicals needed for this experiment are: * Hydrochloric acid - this is the solution that the magnesium will react with, I will be using 10cm� of it and its concentration will be 1.5 molars.

  1. Neutralisation Coursework

    Showing that it is a 1: 1 ratio. In our practical we chose to change a few of the amounts used by our teacher to suit our own experiment. For example we started with 15ml of the base Ammonium Hydroxide.

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

    In this experiment the concentration of the acid will stay constant, and the temperature will vary. The concentration of hydrochloric acid and ethanoic acid that will be used is 0.5M. Once the test tube is connected to the gas syringe, record the temperature of the acid and pull the string to release the magnesium strip.

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