• 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

Rate of reaction of different concentrations of sodium thiosulphate.

Extracts from this document...

Introduction

Science Coursework: Rate of Reaction The aim of the experiment: In this experiment I will investigate how different concentrations of sodium thiosulphate affects the time for the cross on a piece of paper to disappear. The sodium thiosulphate's concentration will vary in the stages of the experiment as proportions of water will be diluted with the chemical to see how it effects the time of the visibility of the cross. Prediction: I predict the higher the concentration of the sodium thiosulphate the faster the rate of reaction therefore shorter the time will be for the cross (x) to disappear. Background Information: Sodium thiosulphate is a liquid so its particles will be in constant motion. Before a reaction can occur between two liquids their particles must collide together in order to create a reaction. It is not enough for the particles to collide, the bonds between the atoms they have to be broken before new molecules can be produced. In liquids and gases their particles are continually moving at various speeds, which then collide in different ways. There are different ways of collisions occurring which have different effects such as 'head on' and 'glancing' collisions. The particles that contain a lot of kinetic energy (at a high temperature) collide with a large force therefore gain a heavy contact with another particle (head on). This is known to be successful and a reaction takes place. Where as a 'glancing' collision the particles have not got enough kinetic energy (at a low temperature) to produce a reaction because the contact is not great enough, so a reaction will not occur. Activation energy is the energy that is needed to be put into the reactants before a reaction will start. If the activation energy is high then the success rate is much less. In chemical reactions, if the activation energy is low, a high proportion of collisions will have enough energy and so the reaction is fast. ...read more.

Middle

Immediately after all of the acid is poured in start the stopwatch. Step 6- One person in the group has to be responsible for the visibility of the cross as the judgment must be unique. Keep a constant watch over the solution to check when the cross is completely covered by the precipitated sulphur. Step 7- As soon as the cross (x) disappears stop the stopwatch and record the reading to two decimal place for more accuracy. Step 8- Drain out the beaker containing precipitated sulphur and rinse the flask with water then wipe with a clean dry cloth. Step 9- Re-do each concentration three times in this exact method. This will increase reliability and the three outcomes for each concentration can be found a mean time. Table showing the results of my experiment. Analysis of my table showing the results of my experiment: This is the table that shows the results I got from my experiment. I decided to choose three trials for each concentration of sodium thiosulphate so the results I receive are more reliable thus giving me a mean time (seconds). The mean time for each of the concentration will help me to plot a graph. The preliminary experiment had only 2 concentrations the strongest (40g/dm3) molarity and the weakest (8g/dm3) molarity but I decided to include 5 different concentrations of sodium thiosulphate so I can see the difference in time for the cross to disappear and also for a better trend. During the process of my experiment I had realised the weaker the solution the slower the rate of reaction so the time increased. In my initial prediction I knew this would happen because of the collision theory. The collision theory can explain these results because the higher the concentration the faster the rate of reaction. My results show between the concentration of 40g/dm3 and 16 g/dm3 the three trials are very close to each other but the concentration 8g/dm3 the three trials aren't as close. ...read more.

Conclusion

My first graph, time taken for the cross to disappear shows a perfectly smooth curve with no anomalous points. My second graph, how the concentration of sodium thiosulphate influences the rate of reaction displays that all five plots create a straight line going upwards which intends again that my evidence is reliable and very accurate. Both my graphs suggests that my evidence is accurate and sufficient to support the conclusion. The conclusion to my experiment is in higher concentrations of sodium thiosulphate the faster the reaction is therefore the quicker the time for the cross to disappear. I would extend my investigation by carrying out more concentrations of sodium thiosulphate and maybe using other chemicals such as potassium thiosulphate to contrast the rate of reaction between the two. This would let me know how different chemicals influence the rate of reaction and this can also help me to compare the results that would give me a far better conclusion. In order for this to happen I would have to keep everything constant for both chemicals like temperature and the concentration of hydrochloric acid. Another way to extend my investigation is maybe by including a catalyst in the solution of sodium thiosulphate and hydrochloric acid. This would let me go more into depth of the topic, rate of reaction. The catalyst would let me see exactly how it influences the rate of reaction and how much of the time for the cross to disappear it actually alters. I think the catalyst would speed up the rate of reaction because it would provide a boundary where the particles meet and collide, this should certainly increase the rate of reaction. The catalyst would allow particles to react even if they collide with only low energy, this will make successful collisions more likely. This would happen by the catalyst fixing particles on its surface that will make the chances of collisions more likely. The more collisions there are the faster the rate of reaction. This would certainly precipitate sulphur faster that will make the cross disappear quicker as well. ?? ?? ?? ?? 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 Classifying Materials 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 Classifying Materials essays

  1. Marked by a teacher

    In this CDA I will write about how plastic bags are made, why plastic ...

    Handles can be added now with a heat press process, or moulded straight on to the bag. 7. The remaining, unused plastic is then recycled to make more plastic bags. Are plastic bags good for the environment? Plastic bags are not good for the environment.

  2. The rates of reaction between CaCO3 and HCL

    24.94 24.69 00.32 165 24.84 24.25 24.92 24.67 00.34 180 24.84 24.25 24.92 24.67 00.34 195 24.83 24.24 24.91 24.66 00.35 210 24.82 24.23 24.90 24.65 00.36 225 24.81 24.22 24.90 24.64 00.37 240 24.80 24.22 24.89 24.64 00.37 Analysis: Trends and patterns: The lines shown on the graph are

  1. Calcium carbonate reacts with dilute hydrochloric acid according to the equation below

    On each of these graphs I will calculate the initial rate of reaction. I will do this for the first 15 seconds, because this is when the concentration of acid is most accurate. The rate of reaction is calculated by dividing the change in mass by the number of seconds it changed in.

  2. Rate of reaction of hydrochloric acid on magnesium.

    It is important for the temperature to be the same, as it will have a massive influence to the amount of collisions. If the temperature is increased then the particles motion will increase as will there for the contacts between the opposite particles will be heavy and in parallel the success rate would have increased making the reaction time faster.

  1. Do different fuels produce different amounts of energy?

    Set up the experiment as the diagram shows 2. Weigh and record the spirit burner's weight 3. Put the spirit burner back to position and light it 4. When the temperature of the water has increased by 35 �c, put the fire off 5. Weigh and record the spirit burner's weight 6.

  2. Free essay

    Periodic table

    CaCl2 which means 2 chlorine ions for every calcium ion. Water covalent bonding: O / \ H H = The hydrogen atoms share one electron each and the oxygen needs two to get a full outer shell - Single Bond - shares only one electron to gain a full shell.

  1. Our experiment consisted of two samples of water containing unknown substances, and our objective ...

    11. We need to get rid of the water so all that's left is the mystery solid. Therefore, we need to put the evaporating basin (now containing the sample of water) back onto the gauze. 12. Evaporation takes places and the water escapes the evaporating basin by turning from liquid to gas.

  2. Redox reactions and the halogens.

    Three basic types of forces; Van der Waals forces - between any molecule Dipole - dipole attractions - between polar molecules Hydrogen bonding - between certain dipole molecules Van der Waals forces (temporary dipole - dipole) - weakest intermolecular attraction - occurs in all molecules Happens because electrons in the

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