• 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
  13. 13
    13
  14. 14
    14
  15. 15
    15
  16. 16
    16

My aim is to see that if I change the concentration of Hydrochloric acid for each experiment I will see an increase or a decrease in the rate of reaction between the Hydrochloric acid and magnesium ribbon.

Extracts from this document...

Introduction

AIM My aim is to see that if I change the concentration of Hydrochloric acid for each experiment I will see an increase or a decrease in the rate of reaction between the Hydrochloric acid and magnesium ribbon. Prediction My prediction is that the higher the concentration of the acid then the higher the rate of the reaction will be. I am stating this because of collision theory (see introduction). * The higher the concentration of acid, then the higher the number of acid particles present per 10cm� of acid. This means that there should be more collisions per second, which means there should be more successful collisions per second, so the rate of reaction should increase. If I double the concentration of acid from 1 molar hydrochloric acid to 2 molar hydrochloric acid then I should expect to see the rate of reaction double. This is because there are twice as many acid particles in 2 molar hydrochloric acid than 1 molar of hydrochloric acid, so there should be twice the amount of collisions per second and because there are twice the amount of collisions per second then there should be twice as many successful collisions per second, which should result in an increase in the rate of reaction. Plan * I intend to react 2 cm lengths of magnesium ribbon with 10cm� of Hydrochloric acid of varying concentration. * I will measure the rate of reaction by timing the experiment from when I drop the magnesium in to the boiling tube with the hydrochloric acid. Observing the magnesium until it has completely dissolved. I am also going to shake the boiling tube. ...read more.

Middle

1) Temperature of the Hydrochloric acid. Why rate changes with temperature? If the temperature of the acid is different each time the reaction will not be fair. At low temperature the particles do not have much energy. When Substances are given heat the particles take in energy. When energy is given to particles they move faster and collide more often. This will give a successful collision. The rate of reaction increases and is faster. Low Temp High Temp Acid Magnesium 2) Type of acid used If I change the type of acid then the rate of reaction would change. Hydrochloric, Sulphuric and Nitric acid would all produce a different rate of reaction, so if I do change the type of acid then all three kinds would produce a different set of results. 3) Concentration of the Hydrochloric acid The more concentrated the reactants, the grater the rate of reaction will be, because the higher the concentration of acid then the more acid particles per 10cm� so more collisions per second there for there will be more successful collisions per second. More acid less acid Acid Water 4) Boiling tube shaken or not shaken. Shaking the Boiling tube whilst the reaction is taking place can alter the rate of reaction because when the reaction is taking place there is already collisions taking place in the Boiling tube. When the particles gain kinetic energy by movement this helps to make the reaction faster. Shaken Not Shaken Acid Magnesium 5) Presence of catalyst. A catalyst is a substance, which can alter the rate of reaction, but remains chemically unchanged itself at the end of the reaction. Catalysts usually speed up the reaction. ...read more.

Conclusion

I decided that it would be impractical to spend time on the low concentrated of hydrochloric acid. I furthermore learnt from my preliminary work that it was sometimes quite difficult to stop timing on the exact moment that the magnesium had dissolved. I decided therefore that I would carry out each experiments three times and find the average time as this would result in more accurate figure. When magnesium reacts with hydrochloric acid, magnesium chloride is formed. I wrote down the equation to show this: Magnesium + Hydrochloric acid = Magnesium chloride +Hydrogen Mg + 2HCl {r} MgCl2 + H2 The equipment I needed for the experiment were: * Stop watch * Water * Hydrochloric Acid 2moler * Magnesium ribbon (2 cm) * Test tube rack * Boiling tube * Ruler * Scissors * Measuring cylinder * Goggles I decided to do the experiment, three times each, using all the information that I gained while I was doing my preliminary experiment. Results Concentration of acid Volume of acid Volume of water Experiment (Time in seconds) 1 2 3 Average (Time in seconds) Rate 1/t 02 molar 10 cm� 0 cm� 15 15 14 14.7 0.68 09 cm� 01 cm� 17 18 19 18 0.56 08 cm� 02 cm� 21 23 24 22.7 0.44 07 cm� 03 cm� 26 25 27 26 0.38 06 cm� 04 cm� 39 40 38 39 0.26 01 molar 05 cm� 05 cm� 57 59 56 57.3 0.17 04 cm� 06 cm� 70 66 69 68.3 0.15 03 cm� 07 cm� 210 225 223 219.3 0.05 02 cm� 08 cm� 532 529 540 533.7 0.02 01 cm� 09 cm� 1178 1180 1195 1184.3 8.4x00-4 0 molar 0 cm� 10 cm� ------ ------ ----- ---------- ----- ...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)

    1.17 40 35 35 36 35.33 0.88 50 35 35 36 35.33 0.71 60 35 35 36 35.33 0.59 1.7 10 25 20 22 22.33 2.23 2.23 20 38 34 33 35.00 1.75 30 38 34 33 35.00 1.17 40 38 34 33 35.00 0.88 50 38 34 33 35.00

  2. Marked by a teacher

    Investigation of the rate of reaction between Magnesium and Hydrochloric acid

    4 star(s)

    and only one result needs to be recorded (the time it takes for the mark to disappear.) Disadvantages: This method only works if the solution is see-through. Also people might disagree when the mark has appeared or not. Preliminary Work The reason why I need to do Preliminary work before

  1. A reaction between Hydrochloric Acid and Magnesium ribbon.

    Before moving on the next concentration I will make sure that I clean the conical flask with water. The factors, which may affect how well the experiment works, are how quickly the ribbon is placed in and the stopwatch pressed.

  2. The effect of temperature on the rate of reaction between magnesium ribbon and hydrochloric ...

    This could have caused big errors in the reliability of my results. For example, the time of the chemical reaction was measured to an accuracy of 1 second. Thus, the percentage error on measuring the reaction lasting ... seconds for ..�C is ...%.

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

    To prevent this I coiled up the magnesium and dropped it in so that it pierces the acid, so that it's all covered. Lastly, I thought that it would be a good idea to rinse out the beaker after experiment.

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

    However, as I am not going to rely solely on the results of my preliminary investigation to conclude it, I am not going to pay so much attention to things like fair testing, although I will try and conduct the investigation as fairly as I can.

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

    Apart from trying to find the optimum rate of reaction I also have to find out how to keep the temperature change down. This is because as the reaction is taking place the temperature will rise because the reaction is exothermic, and this could cause my results to be inaccurate

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

    The Maxwell-Boltzmann distribution theory tells us that for every 10�c rise in temperature the reaction rate doubles, meaning double the amount of particles have the energy to perform effective collisions. Evaluation Anomalous results: From looking at the graph I can see that there are three points which do not fit

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