• 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

An investigation of one factor which affects the rate of reaction between Sodium Thiosulphate solution and hydrochloric acid.

Extracts from this document...

Introduction

Steven Mavrou-St. Edmunds School-61423 An investigation of one factor which affects the rate of reaction between Sodium Thiosulphate solution and hydrochloric acid. Na2 S2 O3 (aq) + 2HCl (aq) = 2NaCl(aq) + S(s) + SO2(g) + H2O(l) Introduction: Sodium Thiosulphate solution is a colourless solution and hydrochloric acid is also a colourless solution. When mixed together and then shaken, the solution gets cloudy until it becomes a pale yellow colour and you cant see through the solution. In this assessment I have been asked to investigate one factor which affects the rate of reaction between Sodium Thiosulphate solution and Hydrochloric acid. I will do this by putting a cross underneath my beaker and time how long it takes until I cannot see through the mixed solution. In my investigation I will use my knowledge on the theories of collision and kinetic. I will also use my knowledge on Activation energy and heat energy. Collision theory It is the theory used to predict the rates of chemical reactions, particularly for gases. The collision theory is based on the assumption that for a reaction to occur it is necessary for the reacting atoms or molecules to come together or collide with one another. ...read more.

Middle

4.Measure out amount of distilled water needed into a measuring cylinder. 5.Add distilled water into the sodium thiosulphate. 6.Measure out needed amount of hydrochloric acid into a different measuring cylinder. 7.Place 100cm3 conical flask directly above a piece of paper with a cross on it. 8.Have a stopwatch ready for use. 9.Add the hydrochloric acid to the sodium thiosulphate and distilled water solution. 10.Press start on your stopwatch. 11.Stir the mixed solution at a steady speed until you cannot see the cross through the solution. 12.When you cannot see through the solution press stop on the stopwatch and record your answer. 13.Pour the solution down a fume cupboard and rinse and clean the conical flask so it is fit for use for the next experiment. 14. Now repeat the experiment 5 times. List of Equipment 1. 100cm conical flask 2. 50cm measuring cylinder 3. 25cm measuring cylinder 4. Stopwatch 5. Thermometer 6. Dropping pipette 7. A cross on a piece of paper 8. 1.0 M hydrochloric acid 9. 40g/l sodium thiosulphate 10. Distilled water 11. Fume cupboard for waste products. 12. Safety glasses 13. Lab coat Prediction In my experiment I predict that when I increase the concentration of sodium thiosulphate the rate of reaction will also increase. ...read more.

Conclusion

I would investigate this to see what results I may get by changing a different factor. I would change the concentration of the hydrochloric acid and change the amount of water accordingly and I would keep the amount of sodium thiosulphate the same. Whilst doing all this I would keep the total amount of solution the same throughout. This is a table to show how I would do this experiment AmountofHydrochloricAcid(cm3) 40 35 30 25 20 15 10 AmountofWater (cm3) 0 5 10 15 20 25 30 AmountofSodiumThiosulphate(cm3) 10 10 10 1 10 10 10 TotalAmountofSolution(cm3) 50 50 50 50 50 50 50 I predict that by increasing the hydrochloric acid the rate of reaction will decrease. When I double the amount of hydrochloric acid the number of particles will halve in every cm3. Therefore the amount of collisions will halve per second and therefore the amount of successful collisions will halve, and the rate of reaction will also halve. If I decrease the hydrochloric acid the rate of reaction will increase. When I decrease the amount of hydrochloric acid the rate of reaction will increase. When I halve the amount of hydrochloric acid the number of particles will double in every cm3. Therefore the amount of collisions will double per second and therefore the amount of successful collisions will double, and the rate of reaction will also double. ...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. An investigation into how surface area affects the rate of reaction

    someone else in the lab is using a Bunsen burner, or knocking over equipment that happens to be lying around. we have to be careful because the acid is highly corrosive to our bodies and should be kept away from skin and from our clothes.

  2. What Affects the Rate of Reaction Between Sodium Thiosulphate and Hydrochloric Acid?

    Next, I will get the equipment needed to perform the experiment. I will get certain amounts of Sodium Thiosulphate, and certain amounts of Hydrochloric acid (amounts will vary according to the reaction table). I will place the two reactants into a beaker with a set amount of water, and place the beaker over the black cross.

  1. The purpose of this investigation is to find out the different factors which, affects ...

    This involves two types of theories, the kinetic and collision theory. The kinetic theory states if the movement of particles in a substance increased particles have gained energy, they move around faster colliding with each other this falls in the collision theory.

  2. An investigation into how the concentration of sodium thiosulphate solution affects the rate of ...

    The particles are closer together and have more chance of coming into contact. There is more room in the sealed container so the particles have less chance of coming into contact. Surface area When solids are reacted, the surface area that is exposed to the reactant will greatly affect the rate of the reaction.

  1. Rates of Reaction experiments

    New bonds can form only if the atoms are close enough together to share electrons. Some collisions are not successful. These are called unsuccessful collisions Collisions that lead to products are called successful collisions. A successful collision must happen with a great enough speed, energy and force to break bonds in the colliding molecule.

  2. The purpose of this experiment is to see how the concentration of hydrochloric acid ...

    I have done this as a differ in light intensity will affect the results as this is how I will determine if the reaction has finished. Finally the last variable will be the dependent variable (what your measuring), which is how long it takes for the solution to become cloudy

  1. What affects how quickly sodium thiosulphate solution goes cloudy?

    As I know that there a set number of particles in a given volume of thiosulphate, it is safe to assume that halving the concentration will halve the number of successful collisions. This in turn will double the rate of reaction (as the collisions will be occurring only half as frequently).

  2. How does the concentration of sodium thiosulphate solution affect the rate of its reaction ...

    I will measure the amount of time a black cross drawn on a piece of paper underneath the conical flask takes to disappear. During the reactions I will record the time taken in seconds using a stopwatch for each concentration to react.

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