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

Investigation into what factors can affect the rate of a chemical reaction.

Extracts from this document...

Introduction

An investigation into what factors can affect the rate of a chemical reaction. Section 1 Planning I have been asked it investigate what factors can influence the rate of a chemical reaction. I will be reacting magnesium and hydrochloric acid. To measure the rate of a reaction, I will time how long it will take the reaction to produce 5ml, 10ml, 15ml, and 20ml of hydrogen. There are a number of variables that can affect the rate of my experiment i.e. > Size of the magnesium, this is because there is more surface area: more magnesium is exposed to the hydrochloric acid and therefore more acid can attack the magnesium. > The concentration of the acid, this is because there are more acid molecules in a greater molar of acid and therefore more acid molecules can attack the magnesium atoms. > Catalysts, weakening bond, this will increase the rate of the reaction by lowering activation energy. (A catalyst will not be used in my experiment) > Temperature, this is because heat will give more energy to the reaction and therefore the particle will move around faster causing more collisions between the magnesium atoms and hydrochloric acid molecules. I have decided to investigate how the concentration of the acid can affect the rate of a reaction. ...read more.

Middle

1. Set up the apparatus as shown in the diagram. 2. Measure 30ml of hydrochloric acid using the measuring cylinder. 3. Pour the acid into the conical flask. 4. Measure 3cm of the magnesium ribbon using the ruler. 5. Drop the magnesium into the acid. 6. Quickly put cork into the conical flask. 7. Start stopwatch immediately. 8. Time how long it takes the syringe to fill 5ml, 19ml, 15ml, and 20ml. 9. Record the results in my table. 10. Empty conical flask and wash out. 11. Repeat steps 2 - 10 with a different concentration of acid. 12. Repeat step 2 - 11 six times. Section 2 Obtaining Evidence Below is a table showing the results from my experiment. I tried to make this experiment as accurate as possible. I repeated each different concentration of acid six times and then took and average to make the results more reliable. The results were recorded to the nearest second. Experiment number Concentration (molars) Time takes when hydrogen given off was (seconds) 5ml 10ml 15ml 20ml 1 0.25 49 133 243 333 2 0.25 74 155 247 424 3 0.25 68 180 302 432 4 0.25 55 154 295 364 5 0.25 59 149 274 385 6 0.25 64 175 264 355 1 0.5 24 63 76 81 2 0.5 16 53 76 95 ...read more.

Conclusion

I could improve my experiment by putting the stopper in more quickly; find another, more accurate way of measuring the magnesium' and we could control the room temperature. To extend my experiment I am going to investigate how the surface area can affect the speed of a reaction. I predict that the bigger the surface area, the faster the reaction will be. This is because there will be more magnesium being exposed to the hydrochloric acid. Therefore, more acid will react with the magnesium. Here is a systematic plan to carry out this experiment. 1. Set up the apparatus in the same way as the previous experiment. 2. Measure 30ml of hydrochloric acid using the measuring cylinder. 3. Pour the acid into the conical flask. 4. Measure 6cm of the magnesium ribbon using the ruler. 5. Drop the magnesium into the acid. 6. Quickly put cork into the conical flask. 7. Start stopwatch immediately. 8. Time how long it takes the syringe to fill 5ml, 19ml, 15ml, and 20ml. 9. Record the results in the table. 10. Empty conical flask and wash out. 11. Cut another piece of magnesium 6cm long. 12. Cut the piece in half. 13. Repeat steps 2 - 10. 14. Cut the magnesium into quarters. 15. Repeat steps 2 - 10. 16. Repeat step 2 -15 six times making the pieces smaller each time. Here is a table of my results: Chemistry Coursework 1/7 Amy Blaney ...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. To investigate three factors that affect the rate of cooling a liquid and to ...

    71?C 73?C 78?C 320 seconds 70?C 72?C 76?C 360 seconds 67?C 71?C 73?C 400 seconds 66?C 70?C 70?C 440 seconds 63?C 68?C 67?C 480 seconds 62?C 67?C 65?C 520 seconds 60?C 65?C 63?C 560 seconds 59?C 63?C 60?C 600 seconds 58?C 60?C 58?C 640 seconds 56?C 58?C 54?C 680 seconds

  2. Antacid Investigation.

    I shall do the following: Brush out the reminder of crushed tablet into the water. Instead of letting out 0.5 ml of HCl each time I shall let out 0.2 to make the experiment even more accurate. Spend more time reading the results.

  1. Aspirin Investigation

    Five drops of neutral Fe(III)Cl3 solution were added. A slight colour change was observed, the solution turning pale violet. This indicates that the sample contains a small quantity of salicylic acid and is not 100% pure aspirin. General Equation for FeCl3 Test + 2 OH OFeIII FeIII + + H+

  2. Rates of Reaction

    Catalyst The word catalyst means an added substance, in contact with the reactants, that changes the rate of a reaction without itself being chemically changed in the end. Catalysts increase the rate of a reaction by helping break chemical bonds in reactant molecules and provide a 'different pathway' for the reaction.

  1. An investigation of the factors which affect the reaction of acid rain on limestone.

    This meant that in order to do the 10�C experiment I had to add ice to the water bath to cool it down. It is my opinion that because of the extreme atmospheric heat in the laboratory - about 25 - 30�C at times - that the acid was reheated up after I had cooled it, with the ice.

  2. Rates Investigation - Hydrochloric Acid and Magnesium Ribbon.

    (1) Volume of Gas (ml) (2) Average Volume of Gas (ml) 20 0 2.00 20 71 73 72 18 2 1.80 67 69 68 16 4 1.60 63 56 59.5 14 6 1.40 47 56 51.5 12 8 1.20 37 38 37.5 10 10 1.00 29 26 27.5 These are graphs of my results What happened

  1. A Investigation into the Rate of Chemical Weathering of Marble

    Using smaller pieces of marble would increase the reaction rate because this increases the total surface area which is where the reaction takes place. Increasing the surface area must increase the number of particles of the marble coming into contact with the acid solution.

  2. An investigation into the factors affecting the rate of reaction of indigestions tablets with ...

    different ratios of acid to water to vary the concentration, different quantities of acid were measured into the beakers using a measuring cylinder. This was then mixed to a certain quantity of water to produce 50 cm3 of the acid (5 beakers in different concentrations).

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