• 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 increases overall rate of reaction. * Catalysts lower the activation energy so particles are more likely to react . Catalysts are a substance which is used to speed up chemical reaction without it being used up itself. It provides the reaction to take place at a faster rate.

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

    The Collision Theory is based on the idea that for a chemical reaction to take place, it is necessary for the reacting particles to collide with each other with enough energy to break or form new bonds between the other particles, which is called a successful collision.

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

    Measure out 50cm3 of 0.5m hydrochloric acid. I have chosen this amount as preliminary tests show this amount to be suitable to what I am doing. Any more acid would prove to be a problem, as too much hydrogen would be formed then 100cm3, the maximum range of the gas syringe.

  2. Rates of reactions between HCL and magnesium ribbon.

    diagram), I will cut a piece of magnesium ribbon to 5cm long. To make sure that all the gas given off is collected, I will ask some-one else to start the stop-watch as soon as the magnesium ribbon is in and the bung to the conical flask placed in the top.

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

    Distilled water (cm�) 50 0 40 10 30 20 20 30 10 40 I made the concentrations using hydrochloric acid and dilute water. I measured the liquids using measuring cylinders to make the required concentrations. I then poured the solutions into five beakers and measured the amount of magnesium needed.

  2. The aim of this investigation is to find out the effect of concentration of ...

    wwaa aaw esaaaas ayaa aaba naa kcaa aauk! The graph shows that there is an increase in the rate of reaction as the concentration increases because the graph has it�s largest gradient or it is steepest at this point. When the graph was made into 1/time the result should have been a sraight line graph but it did not turn out this way even though concentration~1/time.

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

    : This enabled us to predict the time taken for the experiment And there fore the graph of Time Taken vs. Concentration: Just before we began to start our coursework we carried out a pilot test in order to aid us in determining what concentrations of acid we were to use.

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

    The above calculation shows that 10.4 dm3 is the minimum amount I need to obtain 100cm3 from 0.10 grams of magnesium. Variables: As in most scientific experiments, variables have to be found and then controlled in order for the investigator to be able to compare results accurately and form reliable conclusions.

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