• 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
  10. 10
    10
  11. 11
    11
  12. 12
    12

Rates of reaction between Magnesium and HCl.

Extracts from this document...

Introduction

Chemistry coursework: Investigate one factor which affects the rate of reaction of magnesium and hydrochloric acid Plan I am going to investigate how the change in concentration will affect the rate of reaction, between magnesium and hydrochloric acid (HCL). To broaden my investigation I will use a wide range of concentrations in order to evaluate the differences. To ensure that my experiment will be carried out safely, everyone involved in the experiment will wear safety goggles at all stages of the experiment, as hydrochloric acid is a corrosive substance, and protective clothing must be worn at all time whilst conducting the investigation. The practical will be carried out in plenty of space, clear of bags and coats. It is also imperative to consider the safety of other pupils that may be close to the practical. Therefore no one who is not involved in the practical shall be allowed in close vicinity of the experiment. Also care will be taken when handling the equipment and the hydrochloric acid, in order to avoid spillages. Avoid skin contact with hydrochloric acid. Wear goggles at all times. Rinse skin thoroughly if contact is made. Hydrogen gas is flammable. Keep magnesium away from ignition sources such as open flames. Wear eye protection; wash acid spills immediately. In this investigation the dependent variable(s) is the amount of hydrogen produced and the time taken, as this is unknown or controlled prior to the experiment. The independent variables in this experiment will be the concentration used, the amount of hydrochloric acid and water used, the temperature, the length of magnesium of magnesium ribbon, as these are controlled prior to the experiment. Accuracy of the measurement will be the hardest factor to keep constant because it is almost impossible to get completely accurate results in an experiment like this with the equipment we are provided with. Human experimental error is a problem because factors like reaction times, eyesight and our own judgement cannot be changed and the do affect the end result considerably. ...read more.

Middle

Then take the average. The variable that I am going to change is concentration. I predict that the order of the fastest reaction to the least would be from the greatest concentration of 1M to the least concentration of 0.1M. The scientific reason behind my hypothesis is that when increasing the concentration of the hydrochloric acid, the numbers of particles present also increase and so increase the chance of collision. There would be more chance of the particles interacting, and so the reaction will proceed at a faster rate. Analysis From the results that I collected it is clear that the concentration with the fastest rate of reaction was that of 1M hydrochloric acid. The slowest reaction was when the concentration was 01.M. Here is the order of the fastest to slowest reaction: Fastest 1.0M 0.9M 0.8M 0.7M 0.6M 0.5M 0.4M 0.3M 0.2M Slowest 0.1M As shown in the results tables, I collected a first set of results, then a second and then averaged the results in order to obtain fairly accurate and reliable result. I was aiming to do collect a third setoff results but due to the amount of time that was available this could not be completed. My prediction that the highest concentration, 1M, would be the fastest reaction was correct, with a total amount of 22.7cm� of hydrogen produced. The reaction was extremely fast during the first 30 seconds, however towards the end of that experiment the amount of hydrogen produced stayed the same, as he 20mm strip of magnesium was used up, and therefore no further reaction could occur. The reason why the highest concentration was the fastest reaction is because when increasing the concentration of the hydrochloric acid, the number of particles present also increases and so increases the chance of collision. There would be more chance of the particles interacting, and so the reaction will proceed at a faster rate. ...read more.

Conclusion

This was especially so for the highest concentration in my investigation of 1M. This did not occur in the low concentration, as the magnesium was slowly reacting with the low concentration acid, and the hydrogen produced was steadily increasing. If I were to repeat this experiment again I would certainly ensure that I would use a substance such as Vaseline to limit the amount of hydrogen escaping. I would also use a more accurate burette, than with 0.01cm� increments, rather than 0.1, as this would enable me to obtain more accurate results, as the results were fairly close together. As well as this I would ensure than more test were done, for example five as oppose to only two. This would then give me more accurate and reliable results. I could take this experiment further by using a different metal such as Zinc and aluminium. I could investigate other different factors that affect the rate of reaction such as temperature or surface area. I could use a fixed amount of hydrochloric acid, and could alter the surface area of the magnesium strip. I could also use the other method of measuring the rate of reaction. Measure the rate at which the chemicals disappear, rather than measuring the rate of products formed. However, this may be an unreliable method, with the equipment available, at this would be based on ones own judgement. A more advanced and technological way, could be to use a particular program that will enable me to collect data that will instantly be put onto graph, and will show how changing the concentration affects the reaction rate throughout the investigation. The investigation could also be extended to investigate other factors affecting the rate of reaction such as catalysts, temperature of the acid or particle size of the magnesium. Such ideas could give more evidence, or extend my investigation in this subject field. ?? ?? ?? ?? Tarik Saif 11Sn ...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)

    leads to an increase in colliding but also, as the energy is increased it then has a higher chance of a collision occurring with sufficient energy. Rate of reaction increases as the temperature increases. The graph displays the minimum energy needed to start of the reaction of to break the bonds to allow the activation energy to work.

  2. Marked by a teacher

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

    3 star(s)

    On page 79 in the relative section this is what I found: "When the temperature is increased the particles all move quicker. If they're moving quicker, they're going to have more collisions." The second relative quote was on the same page: "The rate of a reaction simply depends on how

  1. Marked by a teacher

    In this project I am going to investigate rates of reaction of an indigestion ...

    3 star(s)

    will be more accurate than the gas syringe as I only want to measure the time to the nearest second. Also the gas syringe only has markings every for every 5cm� of gas given off, and therefore it would be easier to measure to a marking on the syringe.

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

    each time the speed at which the acid particles collide with the magnesium ribbon will increase more the higher the temperature goes. This means the acid particles move with more energy, which means they will collide with the magnesium with more energy, which will give more successful collisions per second.

  1. To investigate the effect of the concentration of nitric acid on the rate of ...

    I therefore disregarded the result but have circled it on the graph to identify it as a result which falls slightly out-of-pattern. EVALUATION OF INVESTIGATION: Overall, I think I could call the investigation a success because my results supported my prediction and there were only a few anomalous results, which I have acknowledge and dealt with appropriately.

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

    PREDICTION AND HYPOTHESIS I predict (using information earlier in this section) that as you increase the temperature the rate of reaction will increase. This is because the heat energy, which is supplied to the atoms, is converted into kinetic energy and therefore the atoms move and collide with each other causing reactions.

  1. An Investigation into how concentration affects the rate of reaction between magnesium and hydrochloric ...

    They have a greater chance of colliding. Because there are more collisions the reaction rate is greater. How does temperature affect the rate of a chemical reaction? When two chemicals react, their molecules have to collide with each other with sufficient energy for the reaction to take place.

  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