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

Investigation of the Effect of Changing Concentration on the Rate of Reaction Between Magnesium and Hydrochloric Acid.

Extracts from this document...

Introduction

Investigation of the Effect of Changing Concentration on the Rate of Reaction Between Magnesium and Hydrochloric Acid Apparatus * Hydrochloric acid * Magnesium ribbons * Gas syringe * Clamp and stand * 100cm3 flask * Water * Bung * Burette * Connecting tube * 800cm3 jug Method Set up the diagram shown above using the apparatus given. 50cm3 of HCL should be placed in the flask. It will be of 1mol/dm3 and will vary in concentration each time by diluting it with water to get concentrations of 0.2mol/dm3, 0.4mol/dm3, 0.6mol/dm3, 0.8mol/dm3 and 1mol/dm3. The results of the concentrations will give me a suitable graph. 8cm of mg ribbon will be placed in each concentration of HCL as this length will give me sufficient time to record accurate results, but not too much time that I'm waiting around for the experiment to end. I will record the amount of hydrogen given off every 10secs so I can record a significant change in volume on each recording. Also for each reaction the flask will be placed in a jar full of cold tap water to act as a water bath to keep the temperature constant, as the experiment is exothermic. And to make the results reliable I will repeat each reaction twice, thrice if necessary. Concentration Table Concentration (mol/dm3) Volume of HCL (cm3) Volume of water (cm3) 1.0 50 0 0.8 40 10 0.6 30 20 0.4 20 30 0.2 10 40 Reasons for Method I have worked out that 0.1g of mg will give me 100cm3 of hydrogen. ...read more.

Middle

4 15.5 34 64 84 60 4.5 18 39.5 73 84 70 5 20.5 45 77 84 80 5.5 23.5 49.5 78 84 90 6 25.5 55 80 84 100 6.5 28.5 59.5 82 84 110 7 31 64 82 84 120 8 32.5 69 82 84 Results 2 Time (sec) 0.2 mol/dm3 0.4 mol/dm3 0.6 mol/dm3 0.8 mol/dm3 1.0 mol/dm3 10 2 4 10 16 30 20 2.5 6 14 31 52 30 3 9 20 43 73 40 4 12.5 25 55 82.5 50 5 14 31 64 85 60 5.5 17 37 75 85 70 6 20 42 78 85 80 6.5 23 46 80 85 90 7 26 52 83 85 100 7.5 28.5 57 84.5 85 110 8 31.5 61 84.5 85 120 9 32.5 65 85 85 Average Results Time (sec) 0.2 mol/dm3 0.4 mol/dm3 0.6 mol/dm3 0.8 mol/dm3 1.0 mol/dm3 10 2 5 10 16 28 20 2 7 15 30 51 30 3 12 21 42 72 40 4 13 26 54 82 50 5 15 33 64 85 60 5 18 38 74 85 70 6 20 44 78 85 80 6 23 48 79 85 90 7 26 56 82 85 100 7 29 58 83 85 110 8 31 63 83 85 120 9 33 67 84 85 Analysis The results I gained from each experiment were all very accurate and each set of results proved to be reliable by not being more than 10cm3 away from each other. ...read more.

Conclusion

The best thing that we could have done with the apparatus was to replace it all with new apparatus that had not been used so there was no chemical stains on it and everything that had to move did so very smoothly i.e. the flask and tubing and the syringe. Before we started this experiment we done another experiment to find out what length of mg to use for this experiment and we used a syringe in this experiment so we were able to find out hat by twisting the inner part of the syringe we could loosen it, this turned out to be very useful for this experiment as we were able to increase the accuracy of the results. If we were to do another experiment using another variable I would use temperature as the variable and keep the concentration and length of mg constant. In this experiment I know that the rate of reaction would increase with temperature due to collision theory 'the higher the temp the more energy the particles have to break the bonds and the particles will move faster and more particles will be of activation energy and the percentage of successful reactions will rise'. The problem with this experiment would be that it is very hard to keep the temp constant and a top of the range water bath would be needed. Rates of Reaction Rate of reaction =amount of gas/time (time used must be kept constant) 0.2mol/dm3 Rate=3/30 Rate=0.1 0.4mol/dm3 Rate=12/30 Rate=0.4 0.6mol/dm3 Rate=21/30 Rate=0.7 0.8mol/dm3 Rate=42/30 Rate=1.4 1.0mol/dm3 Rate=73/30 Rate=2.43 Gregory Yalaju 10P ...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)

    This extra push needed for chemical reaction is called activation energy. Strategy Methods of measuring rates of reaction: Collecting and measuring a gas product, we use this strategy to measure the gas by capturing the gas released by the reaction in the conical flask, and then traveling through the delivery tube into the measuring cylinder.

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

    This is when I will react magnesium ribbon with distilled water to show that there is no reaction between magnesium ribbon and water and that the hydrogen gas is evolving from the hydrochloric acid when it is being broken down into magnesium chloride and hydrogen.

  1. Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

    it gives out heat) which means the temperature of the solution will increase. This is because when bonds are broken (in our case hydrogen and chlorine) they use up energy, and when new ones are formed they they give out energy.

  2. How does changing the concentration of hydrochloric acid affect its rate of reaction with ...

    We used 5cm of magnesium for the preliminary experiment. We set up the equipment needed and did the experiment with the five different solutions. While one person put the magnesium into the beaker, the other started timing using the stop watch.

  1. Rates of reactions between HCL and magnesium ribbon.

    have to make sure that I keep the following factors the same:- volume of acid used (cubic centimetres), surface area of the magnesium, length of magnesium. I will also have to make sure that the gas syringe is correctly connected and that it is placed quickly and tightly enough so that no hydrogen gas escapes.

  2. An Investigation into the effect of Acid Concentration on the Rate of Reaction

    Not only did this aid us in working out quantities for our reaction but also in adding further evidence to our prediction. We found that the higher the concentration of acid the larger the rate of reaction, something which we had expected.

  1. Investigating the Effect of Different Concentration Of Acid Rain On The Rate Of Reaction ...

    There is not much which can be done in order to control this variable, the best that could be done is try and obtain all the results on the same day and in one go during a certain time of the day.

  2. Find out the effect of concentration of acid, in thereaction between dilute hydrochloric caid ...

    While we set up the apparatus we kept the reactants separate so that the starting time of the reactants could be measured accurately and for it to be a fair test. We wore safety goggles when we did the experiment, to protect our eyes from the very harmful acid.

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