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


Extracts from this document...


INVESTIGATING THE RATE OF REACTION AGAINST DIFFERENT CONCENTRATIONS OF SODUIM THIOSULPHATE PLAN Aim The aim of this investigation is to examine the rates of reaction, when sulphuric acid and water is added to different concentrations of sodium thiosulphate. I am investigating the time it takes for an 'x' placed under a conical flask of the solution to be obscured. Research 'Rate of reaction' simply depends on how often and how hard the reacting particles collide with each other. The basic idea is that particles have to collide in order to react, and they have to collide hard enough as well. There are many types of reactions. One of the slowest reactions is rusting of iron. Other slow reactions include weathering, like acid rain damage to limestone buildings. A metal (like magnesium) reacting with an acid to produce a gentle stream of bubbles is a moderate speed reaction. A really fast reaction is an explosion, where it's all over in a fraction. There are three ways to measure the speed of a reaction: * Precipitation- this is when the product of the reaction is a precipitate, which clouds the solution. * Change in mass (usually gas given off) - a reaction that produces gas can be carried out on a mass balance. * The volume of gas given off- involves the use of a gas syringe to measure the volume of gas given off. ...read more.


(Make sure the cylinders are rinsed well before use). 3. After measuring everything put the water in a conical flask, place the 'x' underneath it and add the sulphuric acid and sodium thiosulpahate. (Make sure the paper does not get wet). 4. Start clock immediately 5. STOP CLOCK! Record the time it takes for the 'x' to be obscured 6. Repeat each experiment twice according to the measurements in the table. 7. Make sure the cylinders and conical flask is rinsed out after each experiment. OBTAINING EVIDENCE Results Sodium thiosulpahte Water Sulphuric acid Reaction time (seconds) 1st 2nd Average (Seconds) Rate (100/time) 5cm� 20cm� 5cm� 155 167 161 6.2 10cm� 15cm� 5cm� 97 72 84.5 11.8 15cm� 10cm� 5cm� 51 53 52 19.2 20cm� 5cm� 5cm� 39 49 39.5 25.3 25cm� 0 5cm� 33 31 32 31.25 Conclusion. I found out that as the concentration of sodium thiosulphate increased the rate of reaction got faster; hence it took more time for the 'x' to be obscured. From these set of results it shows that my prediction was correct. From my results indicated in the graphs I can see that they agreed with my prediction. I predicted that the higher the concentration of sodium thiosulphate the faster the speed of the reaction, so the reaction time will decrease. I expected that the graphs would look as follows: Time Rate (s) ...read more.


For this experiment all the measurements I used for my actual experiment would be suitable. Sodium thiosulpahte Water Sulphuric acid 5cm� 20cm� 5cm� 10cm� 15cm� 5cm� 15cm� 10cm� 5cm� 20cm� 5cm� 5cm� 25cm� 0 5cm� To ensure the test was fair to contain reliable results I would have to make sure that the equipments were washed and wiped between each experiment. Also I would have to try to move the conical flask with the magnesium in as least as possible as otherwise I could speed the experiment up involuntary. Also I would have to be very careful in measuring the right volumes as this could affect the time. Safety would also be very important in this experiment I would have to handle all the equipment with utmost care, to ensure accidents did not happen. I could use the same apparatus and idea of the method, which I used in my experiment, and repeat each concentration twice to more reliable results. One difference, which I could make to this experiment, is to add the improvements, which I mentioned for my actual experiment. The results which I would expect would be that as I increased the concentration of Sodium thiosulpahte the rate of reaction would also increase, i.e. the reaction time would be less. This is because the more concentrated the solution is the more sodium thiosulphate particles collide with the other particles. This would make the collisions between important molecules more likely. All my research I have carried out from Edexel modular science- revision guide: book one. ?? ?? ?? ?? - 1- ...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. Experiment to Investigate the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate, with ...

    As a result there are less 'particles of reactant knocking about between the water molecules which makes collisions between the important particles', (Chemistry GCSE Double Science Revision Guide Higher Level- Richard Parsons), less likely so there are fewer successful collisions in the same amount of time.

  2. Find out how the rate of hydrolysis of an organic halogen compound depends on ...

    Hal, the reaction that occurs is R ? Hal + X- R ? X + Hal- (Where R represents the alkyl group, and X represents the halogen atom). The structures of the substances, which were investigating are: H H H H ?

  1. Investigating the Effect of Different Concentration Of Acid Rain On The Rate Of Reaction ...

    This variable will make a difference to the reliability of the experiment as an increase in temperature would cause the molecules to collide harder and faster increasing the rate of a reaction and if this were to take place the rate of reaction change which I would be measuring would

  2. The rate of reaction of sodium thiosulpahte and acid.

    Because the collisions have more energy, more of them are successful and so the rate increases. Particle Size and Surface Area By making the particle size of a solid smaller, e.g. by grinding a solid to a powder, we increase the surface area available for particles of another chemical to collide with and react with it.

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