• 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

Investigation to find out how the rate of reaction between Sodium Thiosulphate and hydrochloric acid that is affected by changing the concentration.

Extracts from this document...

Introduction

Magnesium + Hydrochloric Acid Investigation PLANNING Introduction Investigation to find out how the rate of reaction between Sodium Thiosulphate and hydrochloric acid that is affected by changing the concentration. Preliminary Experiment Aim To investigate the rate of reaction between: Sodium Thiosulphate and Hydrochloric Acid by changing the concentration. Apparatus * Beakers - to pour each substance into * Measuring cylinders - to measure the amount of each substance * Stop clock - to time the reaction * Conical Flask - to pour in all the substances and mix together * Paper with a red cross - to watch as reaction takes place * Hydrochloric acid - for the reaction to occur * Water - for the reaction to occur * Sodium Thiosulphate - for the reaction to occur * Pipette - to take a small amount of solution Hypothesis (Prediction) I predict that as the concentration of the sodium thiosulphate increases the rate of reaction will decrease. This is because if the concentration of a solution is increased there are more reactant particles per unit volume. This increases the probability of reactant particles colliding with each other. ...read more.

Middle

The concentration of the acid affects the rate of reaction because, the higher the concentration of the acid (let's say 2 molars) will cause the reaction to happen quicker compared to a less concentrated acid (let's say 1 molar). If the solution is made more concentrated it means there are more reactants colliding between the water molecules, which make the collision between the important particles more likely. In a gas, the pressure simply squashes the molecules together so there are more collisions. On the diagram below, on the left hand side there are less concentration, less particles and slower reaction. However on the right hand side diagram there is more concentration, more particles and quicker reaction occur. For a reaction to occur particles have to collide with each other. Only a small percent result in a reaction. This is due to the energy barrier to overcome. Only particles with enough energy to overcome the barrier will react after colliding. The minimum energy that a particle must have to overcome the barrier is called the activation energy, or Ea. An increase in the frequency of collisions can be achieved by increasing the concentration, pressure, or surface area. ...read more.

Conclusion

Then place a piece of plastic on top of the measuring cylinder, preventing water to spill out. Place a boiling tube on a test -tube rank. The boiling tube must have the magnesium ribbon placed inside it. Then we will pour the Hydrochloric Acid into the test-tube. When pouring the hydrochloric acid into the test tube I will make sure that I wear safety goggles. Start the stopwatch, and take the measurements of the reaction time, until it finally finishes. Then record the results into a table and then find out how to work out the average. I will repeat each experiment to make it a fair test. Results Below is a table in which I will place all of my gathered results at the end of the experiment. Experiment No. Volume of Thiosulphate/cm� Temperature (�C) Volume of Hydrochloric Acid/ cm� Time Taken for Cross to Disappear/s 1 25 60 5 2 25 50 5 3 25 40 5 4 25 30 5 5 25 20 5 I will then be able to analyse the results and see whether my hypothesis was correct or not. If it isn't then I shall investigate further to see where I could have possibly gone wrong. ?? ?? ?? ?? Hemali Amin Chemistry Coursework S4G Pg.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. How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

    jam and so not giving correct results or that the bung was not placed on the top of the side arm tube fast enough which allowed gas to escape. I conducted all three experiments for each temperature at the same time to save time.

  2. The Iodine Clock Investigation

    The first and most obvious point to make regards the order of reaction with respect to H2SO4 and Na2S2O3. It was made clear from early on in the investigation through background knowledge and trial experiments the concentration of these two substances does not have an effect on the rate of the reaction.

  1. An Investigation into how concentration affects the rate of reaction between magnesium and hydrochloric ...

    of the heat is used back up in the reaction to increase the rate of reaction. The more heat produced the faster the rate of reaction; the faster the rate of reaction the more energy needed to brake the bonds between hydrogen and sulphur so that the next stage of reaction can take place.

  2. How does changing the concentration of hydrochloric acid affect its rate of reaction with ...

    31.15 32.2 32.7 33.1 33.4 20 27.0 28.0 28.5 29.25 30.15 31.25 32.1 10 27.0 27.5 27.8 28.0 28.0 28.0 28.0 When the solution had 50 cm� of hydrochloric acid and no distilled water, the reaction took place very rapidly.

  1. Rate of reaction of hydrochloric acid and mangesium ribbon.

    The first is to find out what the initial rate of reaction would be for concentrations 1.25M hydrochloric acid and 1.75M hydrochloric acid as it would be interesting to see how the rate increases compared to 1M hydrochloric acid. Another experiment that I could do is change the type of acid that I use.

  2. An Experiment to Investigate the Effect of Changing the Concentration of Hydrochloric Acid on ...

    Reading 2 (s) Reading 3 (s) Average Reading (s) Rate of Reaction (arbituary units) 0 none none none none none 0.2 78 39 54 57 0.02 0.4 38 47 28 38 0.03 0.6 45 34 53 37 0.03 Control Variables I need to explain how and why I kept key variables other than hydrochloric concentration constant.

  1. Experiment to investigate how changing the concentration of hydrochloric acid affects the rate of ...

    If a lot of bubbles come out of the reaction then I will have to come up with a solution to make sure that the bubbles do not get out of the beaker. Background Knowledge A chemical reaction is a process by which one or more substances called reactants changes into or more other substances, called products.

  2. Investigating how changing the concentration of hydrochloric acid affects the rate of its reaction ...

    The rate of a reaction can be explained by the collision theory. The collision theory states that the rate of any reaction is dependent upon how hard or often the reactants collide with each other. This rate can be measured in three main ways: Precipitation, Change in mass -usually when

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