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

Rate of Reaction - Sodium Thiosulphate and Hydrochloric Acid

Extracts from this document...


Sodium Thiosulphate Coursework Introduction I have been asked to investigate the effects different factors such as concentration and temperature have on the rate of reaction The rate of reaction is the loss rate of a reactant or the rate of creation of a product during a chemical reaction and it can be measured by dividing one by the time taken for the reaction be completed. Collision Theory states that an increase in concentration, temperature, surface area and the use of a catalyst in a reaction will either increase the rate of reaction by increasing the rate of collision between reactant particles, increase the success rate of collisions between the reactants or both of these reactions, there is also another factor which effects the rate of reaction, but is only applicable in gasses, that factor being pressure. I have chosen to investigate the effects of Concentration on rate of reaction, as it is the most accurately achievable while still challenging factor to change. Method: Equipment- 1x conical flask 2x 50ml measuring cylinder 1x 10ml measuring cylinder 1x pipette Sodium Thiosulphate Hydrochloric acid Water Stop clock Safety goggles Plain paper with a black cross on it. Add 10ml of HCL to a conical flask, by All procedures will be undertaken with safety goggles on. After assembling all of the equipment I will pour as close to 10 ml of hydrochloric acid into the 10 ml measuring cylinder, using the pipette to get the amount as ...read more.


The range of results does seem to be large enough, with three sets appearing to give me a reliable set of results and confirming that the results I do have are close enough. Sodium Thiosulphate (ml) Water (ml) Hydrochloric acid (ml) Time taken for reaction in seconds Test 1 Test 2 Test 3 Average 50 0 10 22.57 24.46 23.53 23.52 45 5 10 25.43 28.24 26.65 26.77 40 10 10 29.27 31.12 32.53 30.97 35 15 10 33.31 55.15 53.15 47.20 30 20 10 62.09 59.49 60.32 60.63 25 25 10 72.16 76.28 75.04 75.49 20 30 10 96.14 101.96 102.07 100.06 Above is the graph showing initial results, with the questionable results being the 15ml Water to 35ml Sodium Thiosulphate results. Bellow you will be able to the results with the new results on, the average is also marked on to this to show how close together the results are and the actual table containing these results (both original and re-dos) is also attached. Since on the lower graph all sets of data are within 5% of each other for time we can assume they are reliable as well as accurate. Sodium Thiosulphate (ml) Water (ml) Hydrochloric acid (ml) Time taken for reaction in seconds Test 1 Test 2 Test 3 Average 50 0 10 22.57 24.46 23.53 23.52 45 5 10 25.43 28.24 26.65 26.77 40 10 10 29.27 31.12 32.53 30.97 35 15 10 40.82 41.21 39.36 40.46 30 20 ...read more.


Using my first graph I would say that the original Results were fairly accurate in their writing down, as we can see from the markings being exactly where they should be but that the testing could well have been a bit inaccurate, with the method making collection of accurate data rather tricky. The reliability of the First set of results is all good seemingly except from the 70% concentration tests which all appear to be unreliable, despite being done at separate times separated by other results, we can tell they are unreliable as they are all outside 5% of each other except for the upper two, which are just inside 5% of each other's values, despite major discrepancies with the lower value and where they should be following the rest of the graph. The second Graph however shows an identical or nearly identical level of accuracy with a better level of reliability due to most results being where they should be and as closely grouped as they should be. Due to the overall reliability and accuracy of my final results, which support the theory that rate of reaction increases as concentration increases I would say it entirely valid to say that my results are such as to allow me to confirm that Collision theory does work and concentration is a factor in rate of reaction. ?? ?? ?? ?? Page | 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

Here's what a teacher thought of this essay

3 star(s)

This is a reasonable experiment write up which has produced a good set of results. The evaluation of the method is short and somewhat superficial. More detail is required in order to reinforce the analysis and evaluation. 3 Stars.

Marked by teacher Louise Star 21/06/2013

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

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    The investigation has to be done in a fair manor otherwise the results would be inaccurate and the conclusion would be incorrect. The variables, which must be kept constant, are: 1) Temperature When particles are heated they gain energy. Raising the temperature causes the particles to move around more often

  2. How does temperature affect the rate of reaction between sodium thiosulphate and hydrochloric acid?

    Graphs will then appear on the computer of light level against time show exactly how quickly the reactions occurred.

  1. Investigating the rate of reaction between sodium thiosulphate and hydrochloric acid

    Below is the relevant equation: - Sodium thiosulphate + hydrochloric acid sulphur + sulphur dioxide + sodium chloride + water. Na2S2O3 (aq) + 2HCl (aq) S (s) + S2O (g) + 2NaCl (aq) + H2O (L) Taking into consideration all of the above points, I believe that the graph of

  2. A-Level Investigation - Rates of Reaction – The Iodine Clock

    5 5 8 8 H2O2 10 10 10 10 15 20 10 20 H2SO4 5 5 5 5 5 5 5 5 Starch 1 1 1 1 1 1 1 1 Time (secs) 16 30 83 235 106 84 102 52 RESULTS: 1 2 3 4 5 6 7 Volume (ml)

  1. The Iodide - Persulphate Reaction: Determining the Effect of Concentration on Reaction Rate

    Knowing that the concentration of S2O8-2 was linearly proportional to the rate constant, we can see in the results that the relationship is very close to being linear, but there is some variation. This can be explained by the ionic strength factor.

  2. Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate.

    Concentration It is the concentration that I will be investigating and is not therefore a variable that needs to remain constant. Prediction I predict that as the concentration of the sodium thiosulphate increases, the time taken for the cross to disappear will decrease.

  1. The Disappearing Cross

    9 9 55 9 9 8 8 60 8 8 8 8 65 6 6 5 6 70 4 4 5 5 From my results I can conclude that as the temperature of the hydrochloric acid rises, the rate for reaction also gets higher.

  2. Iodine Clock Reaction

    Thus each Well had a total volume of 10 drops in it, and each Well from 1 to 10 had a decreasing concentration of KIO3. Of course distilled water was used so as to prevent reactions that might have occurred between salts in regular water and the actual reactants of the reactions.

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