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

My aim in this experiment is to react hydrochloric acid with magnesium in different concentrations to see if gas will be produced quicker or to see a change in rates of reaction.

Extracts from this document...

Introduction

Planning My aim in this experiment is to react hydrochloric acid with magnesium in different concentrations to see if gas will be produced quicker or to see a change in rates of reaction. I am going to wear goggles as a safety precaution as the acid may end up in an eye. As another precaution I am going to be careful when handling the acid and magnesium and I will not eat the magnesium or drink the hydrochloric acid. Method I am going to make sure that this will be a fair test. To do this I am going to use the correct amount of acid in each experiment and I will use the same amount of magnesium in each experiment as well. We are going to change the concentration of the acid by adding 5cm cubed of acid in the first and 0cm cubed of water , in the second I will change the concentration and use 4cm cubed of acid and 1cm cubed of water, in the third I will use 3cm cubed of acid and 2cm cubed of water, in the fourth I will use 2cm cubed of ...read more.

Middle

22 24 23 25 50 21 23 24 25 25 60 21 23 24 25 25 3CM Cubed HCl 2CM Cubed H20 Time (secs) Volume Of Gas 1 2 3 4 5 0 0 0 0 0 0 10 13 8 9 10 7 20 20 13 14 15 13 30 23 18 18 17 19 40 25 22 23 22 27 50 25 25 26 24 27 60 25 28 29 28 29 2CM Cubed HCl 3CM Cubed H20 Time (secs) Volume of Gas 1 2 3 4 5 0 0 0 0 0 0 10 8 15 8 12 15 20 15 22 14 19 22 30 23 24 18 25 28 40 25 26 23 28 30 50 28 29 26 30 37 60 32 33 26 31 40 1CM Cubed HCl 4CM Cubed H20 Time (secs) Volume of Gas 1 2 3 4 5 0 0 0 0 0 0 10 7 6 8 8 5 20 12 10 13 15 10 30 17 15 20 21 14 40 20 19 23 21 17 50 23 24 23 22 20 60 25 26 24 27 21 Analysis The lines on my graph show the different rates of reaction of different concentrations of hydrochloric Acid with 3cm of Magnesium. ...read more.

Conclusion

the average amount of gas released was 32.5cm3 of gas. On the fifth and final reaction (1cm3 HCl 4cm3 H2O) the average amount of gas released after one minute was 24.6cm3 of gas. The reaction was between Hydrochloric acid(HCl) and Magnesium(Mg). This is what the reaction was: Mg+2HCl MgCl2 + H2 Evaluation This experiment went quite well even though in the experiment some things went wrong. We think the results went wrong because we let some gas escape (by accident) on some of the reactions and not (the way it should have been on all) on the rest of the reactions. The beginnings of the reactions were correct but because of the loss of gas the ends of the lines turned out incorrect. The lines on the graph were, I think, near enough to what they should have been and I would expect others to get almost the same as what I got for the lines on the graph. If I could have done this experiment again I would have tried to put the lid on at the same time each time that I did the experiment. The experiment was a success apart from the loss of gas but I think it was great. ...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. Antacid Experiment.

    I have to know the relative formula mass of the active ingredient, which was calcium carbonate, magnesium carbonate, or sodium bicarbonate. I also had to know the mass of the antacid tablet and the moles of the hydrochloric acid. Once I find out the relative formula mass of the active

  2. The aim of this experiment is to determine the rate of reaction between thiosulphate(Na2S2O3) ...

    Once the solution has been put into the test-tube, I will measure out the correct amount of calcium carbonate (marble chips) on a set of scales. In order to have the most accurate results possible in this experiment, it is important to have marble chips of equal mass for each experiment.

  1. Investigating rates of reactions. The reaction I am going to be looking at is ...

    * Next I mixed my five different concentrations of hydrochloric acid and distilled water. * I then poured the first concentration into the conical flask, added one strip of magnesium and put a bung on the flask. * I then started the stop watch.

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

    the water of the ice cream tub and attach it to the clamp. I used cling film instead of other substances that I could have used because it is light which means that it just sits on top of the surface of the water and does not sink into it.

  1. See how different concentrations of Hydrochloric acid change the rate of reaction with a ...

    When the two chemicals react a displacement reaction will take place and the magnesium will displace the hydrogen in the hydrochloric acid forming magnesium chloride and hydrogen gas. Reactivity Series K (potassium) Na (sodium)) Li (lithium) all too dangerous to react with a strong acid Ba (barium) Ca (Calcium) ..

  2. The Rates of Reaction of Metals with Acid.

    k represents the 'rate constant' which at a given temperature equals to the rate of the reaction, which is directly proportional to t-1, where t is the amount of time taken for the reaction mixture to dissolve the metal. If we plot 1/Temperature against log(1/Time), the gradient of the graph will be equal to -EA/R.

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