• 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

The aim of this experiment is to find out how different concentrations of Hydrochloric Acid and Distilled water affect the rate of reaction between Hydrochloric Acid and Magnesium.

Extracts from this document...

Introduction

Chemistry Coursework Aim - The aim of this experiment is to find out how different concentrations of Hydrochloric Acid and Distilled water affect the rate of reaction between Hydrochloric Acid and Magnesium. Plan Method In the reaction between hydrochloric acid and magnesium ribbon, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. In my experiment I am going to measure the amount of gas given off with different concentrations of hydrochloric acid and distilled water reacting with a 10cm length of magnesium ribbon The chemical reaction takes place when the magnesium ribbon comes into contact with the hydrochloric acid. The products that are formed during this reaction are hydrogen gas and magnesium chloride. The formula equation for this experiment is: 2Mg(s) + 2HCl(aq) 2MgCl2 + H2 Magnesium + Hydrochloric acid Magnesium Chloride + Hydrogen I used five different concentrations which were 1 mole/dm3, 0.8 mole/dm3, 0.6 mole/dm3, 0.4 mole/dm3, and 0.2 mole/dm3. I put the hydrochloric acid and distilled water mixture into a conical flask and add the magnesium ribbon. Next I sealed the conical flask with a rubber bung which had connected to it a tube which went to the gas syringe. Every ten seconds I measured the amount of gas given off by the magnesium and hydrochloric acid and recorded them. ...read more.

Middle

I predict my most accurate results will be the 0.2M and 0.4M solutions because the rate of reaction will be slower. Gas will be given off slowly and not as quick as the higher concentration solutions. The graph below indicates what I think the graph should look like. According to my CGP revision guide the more reactive the metal (in my case magnesium ribbon) the faster the reaction will go. The quicker the reaction the more hydrogen gas will be produced. Therefore in the higher concentrations the gas produced will be greater than the gas produced in the more diluted concentrations. Results These are the results I took during my experiment. They are set out in an easy to read clear table as shown below. The averages are shown in red. Time (S) 1 mole/dm3 0.8 mole/dm3 0.6 mole/dm3 0.4 mole/dm3 0.2 mole/dm3 10 80,85,90 85 45,55,40 47 35,32,30 32 15,13,14 14 2,2,2 20 98,98,98 98 79,83,78 80 70,73,75 72 27,26,26 26 5,5,5 30 98,98,98 98 81,83,82 82 90,91,93 91 42,41,40 41 9,9,9 40 98,98,98 98 81,83,93 86 92,93,94 93 53,51,52 52 11,11,11 50 81,85,94 87 94,94,95 94 65,63,64 64 13,13,13 60 94,96,96 95 73,72,72 72 16,16,16 70 96,96,96 96 82,80,81 81 18,18,18 80 87,87,87 87 19,19,19 90 90,89,89 89 21,21,21 100 92,91,91 91 24,24,24 110 93,92,92 92 25,25,25 ...read more.

Conclusion

Evaluation As the concentration of hydrochloric acid increases the rate of reaction increases. My evidence is consistent with no obvious anomalies. I think I got no anomalous results because the experiment I carried out was simple and little could go wrong. I could make a number of improvements to my experiment to acquire even more accurate results. I could of taken more results to get an even accurate average. I could do more in between results. For example I could do concentrations such as 0.1M, 0.2M and so on to 2M covering a wider range of concentrations. My results are accurate and enable me to come to a reliable conclusion that as concentration of hydrochloric acid the rate of reaction increases. Changing one of my variables could lead to an increase in reliability, I could change the mass of magnesium which would result in a larger amount of gas given off. I could increase the surface area of magnesium, Increasing surface area should increase the speed that the hydrogen gas is given off as well. I could use better equipment in my experiment. I could change the gas syringe or one with clearer readings and one that shows all the readings going up in 5cm 3 instead of one going up in 20cm 3. ...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

    The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric ...

    4 star(s)

    Results concentration mol Time (secs) Volume of H2 gas given off in the inverted measuring cylinder (cm3)magnesium (1.5 cm) Average rate (cm3s-1) Fastest Rate (cm3/s) Rep 1 Rep 2 Rep 3 Average 2 10 24 24 24 24 2.40 2.40 20 34 33 37 34.67 1.73 30 35 34 36

  2. Marked by a teacher

    Investigation of the rate of reaction between Magnesium and Hydrochloric acid

    4 star(s)

    Sixth test: Hydrochloric acid 0.4 molar (50 ml) and calcium carbonate powder (0.5 grams) Hydrochloric acid 0.4 molar (50 ml) and calcium carbonate powder (0.5 grams) Seconds (s) Gas produced (cm3) 0 0 30 16 60 19 90 22 120 28 150 31 180 31 210 32 240 32 This worked really well.

  1. Marked by a teacher

    How dose temperature affect the rate of reaction between magnesium and hydrochloric acid.

    3 star(s)

    To investigate how temperature rices in different amounts of acid with different lengths of magnesium carried out a little experiment and collected data that helped to solve this problem and decide on what the amounts should be in the finally practical.

  2. Investigating the rate of reaction between Magnesium Ribbon and Hydrochloric Acid.

    the level off as all the reactant is used up, which in this case is at 100cm3, this shows that there is a relationship between the amount of hydrogen produced and the concentration of the acid. The graphs are a visual image showing me how quickly the hydrogen was produced.

  1. How does temperature affect the rate of reaction between Magnesium and Hydrochloric acid.

    in with the others, they are not on the line of best fit. They are at 20� where the rate is 20, 40� where the rate is 48, and 50� where the rate is 37. On the results table in my observation, the only apparent anomalous result is at 50�

  2. Determine the rate equation for the reaction of hydrochloric acid with magnesium metal, and ...

    This would eliminate the need to place in end of the delivery tube in the gas collector, so there would be no gas lost in any of the experiments. In this way I could obtain a much more accurate set of results, and therefore a more accurate figure for the order of reaction and rate constant.

  1. How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

    as the temperature change will heat up the acid and give the acid particles more energy so they will move faster and collide with the magnesium with greater force causing more successful collisions per second. To show that the hydrogen gas is not being given of from the water in

  2. Finding the effect of concentration on the rate of reaction of magnesium ribbon with ...

    In the experiment I found and confirmed my results to prove my predications and theory, for the effects of concentration on the rates of reaction. My predictions were that as concentration increases so did the rate of reaction, so that an experiment of 2 moles would be faster and double the speed of a 1-mole reaction.

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