• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11
  12. 12
  13. 13
  14. 14
  15. 15

Investigating rates of reactions. The reaction I am going to be looking at is between magnesium and hydrochloric acid.

Extracts from this document...


N kbistry Coursework - Rates of reaction Introduction I am going to be investigating rates of reactions. The reaction I am going to be looking at is between magnesium and hydrochloric acid. Key Variables 1. Temperature of solution) 2. Concentration of reactant 3. Surface area of a solid 4. Use of catalyst 5. Light Key variable for investigation Concentration of reactant Factors to be controlled * Temperature - This cannot be completely controlled because it depends on the room temperature at the time * Surface area of magnesium strip - This can be made very accurate by cutting the magnesium strips the same length, but this cannot be 100% accurate. * Volume of reactant - I can also make this very accurate but it would be very difficult to get the volume of each concentration perfectly accurate. Prediction I think that if I half the concentration of the reactant then the reaction will take twice as long. Reason The reason I have made my prediction the way I have is because I have recently done an experiment using calcium carbonate which gives off carbon dioxide. I found that the more concentrated the solution was with hydrochloric acid the faster the reaction was. Another reason for making my prediction is because of the collision theory. ...read more.


I thought the first 5 concentrations worked well and I am going to use these in my real experiment. Obtaining precise results In my real experiment I am going to try obtain precise and reliable results. To make my readings as precise as possible I am going to start the stop watch 10 seconds before I drop the magnesium into the concentrations of hydrochloric acid so that I do not have to worry about starting the stopwatch.. I am also going to be very careful in pouring the right volumes and concentrations I am using. I will also be very precise with measuring the surface area of each strip of magnesium. To make my results even more accurate I will repeat the experiment. Concentrations 7. 50ml of hydrochloric acid. (2mol/l) 8. 40ml of Hydrochloric acid and 10ml of distilled water. (1.6mol/l) 9. 30ml of hydrochloric acid and 20ml of distilled water. (1.2mol/l) 10. 20ml of Hydrochloric acid and 30ml of distilled water. (0.8mol/l) 11. 10ml of Hydrochloric acid and 40ml of distilled water. (0.4mol/l) 12. 50ml of distilled water. (0mol/l) Results Below is a table to show the results of my experiment with concentration 1. (2moler) Time Run 1 Hydrogen given off in cm3 Run 2 Hydrogen given off in cm3 Average Hydrogen given off in cm3 0 - - - 10 40 42 41 ...read more.


I believe this is because I carried out m experiment carefully and made sure I did not make any mistakes which could of lead to and odd results. The only problem that I came across in my experiment was the amount of time I had to do it in. I overcame this by doing some of the experiment in my lunch hour. The only problem that arose in my method was reading the amount of hydrogen being given off from the syringe. This was a weakness to the accuracy of my results. I believe that the strengths in my method were the organisation of my equipment and the measuring of my solutions. My results seem very reliable but there is some ways in which I could of made them more reliable. I could of got somebody else to take the stopwatch and tell me when to read the measurements from the gas syringe. This would have been much more efficient. I could of also done more repeats to make my results more reliable. I think that my results are sufficient to form a firm conclusion because they show clear trends in my tables and in my graphs. I believe I have sufficient evidence to form a firm conclusion but to be sure I should do more repeats. Further work I could do is to try more concentrations of hydrochloric acid. Chemistry coursework - Rates of reactions Jamie Hannath 11JWT ...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 Aqueous Chemistry 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 Aqueous Chemistry essays

  1. See how different concentrations of Hydrochloric acid change the rate of reaction with a ...

    Concentration (M) 1st Time (Sec) 2nd Time (Sec) 3rd Time (Sec) Average Time (Sec) 0.5 770 781 762 771.00 1.0 732 723 700 718.33 1.5 35 40 35 36.66 2.0 27 32 36 31.66 2.5 18 18 19 18.33 Results for 2nd Experiment Concentration of Hydrochloric Acid (M)

  2. The Rates of Reaction of Metals with Acid.

    Similarly, some rates of reaction are proportional to the volume of a chemical, or the concentration of a solution. Reactions in this category include most uncatalysed inorganic reactions that have their rates dictated by the rate of molecular collisions. Others, normally enzyme-based biological processes, would start off appearing to be

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    If the end point had not been reached, (i.e. the solution did not appear as dark in colour as the others at the end point) the average titre point would be lower; therefore the concentration of Iron (II) would appear lower suggesting that the solution was less concentrated. If either of these had occurred the redox titration would have appear less accurate.

  2. Rate of Chemical Reaction between Magnesium and Hydrochloric Acid

    a popping sound when it came into contact with the flame on the splint. To see how much magnesium and hydrochloric acid I need in my actual experiment I have devised the following mole equation. Mg + 2HCL MgCl2 + H2 1 mole + 2 moles 1 mole + 1

  1. An Investigation to show how concentration changes the speed of reaction between magnesium and ...

    As a lower concentration means fewer molecules this means on average fewer molecules have activation energy for the reaction. The activation energy (Ea) is the energy each of the molecules must have in order for bonds to break and for the reaction to initiate.

  2. Investigation looking At the Speed of Reactions

    Hypothesis If the concentration of an acid increase than output of gas will also increase. When the acid has a high concentration that means in that solution, compared to a dilute one there are more particles available to react with therefore the amount of times they will collide with the each other is more.

  1. Investigating the Rates of Reactions

    I will keep the experiment fair by making sure the conical flask I use, is always washed and dried after each experiment so that there won't be too much or too little of a reactant in the solution because this could change the concentration of water and sulphuric acid.

  2. I am investigating the rate of reaction between magnesium and hydrochloric acid.

    in the casting of metals; and as a getter, a substance that achieves final evacuation in vacuum tubes. The estimated world production of magnesium in 1989 was 350,000 metric tons. The estimated United States production in the same year was 148,000 metric tons.

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