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

Chemistry rate of reaction coursework

Extracts from this document...

Introduction

Chemistry Plan I am going to produce a piece of coursework investigating the rate of reaction, selecting a variable to see how this affects the rate. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product. The rate is measured by dividing one by the time the reaction took to take place. There are five factors that affect the rate of reaction: Temperature Concentration (of solution) Pressure (in gases) Surface area (of solid reactants) Catalysts I have decided to investigate the effect of concentration on the rate of reaction as I feel that it is manageable to measure, will show clear results and is much more practical than the other five variables. Both the Sodium Thiosulphate and Hydrochloric acid are soluble in water; therefore the concentration of either can be changed. However I have chosen to vary the concentration of the Sodium Thiosulphate as it is available to me in larger amounts and is more practical for my investigation. Also whilst changing the concentration it is vital that all other variables remain consistent throughout the experiment. I will not be using room temperature as I cannot control it and this could cause improbabilities within my investigation. ...read more.

Middle

25cm3, 20cm3 etc from the burette into a test tube * Next measure out the amount of water that was needed e.g. 5cm3, 10cm3 etc from the burette into a test tube. * Put both of the test tubes into a test tube rack. * Put the test tube rack into the water bath at a temperature of 40oC so the temperature doesn't affect the results as it is also a variable. * Wait ten minutes to insure that both of the substances are at 40oC. * Next take both of the substances out and put the beaker on top of the cross on a piece of paper, pour both the water and the Sodium Thiosulphate into the beaker. * Start the stopwatch once you have poured in both substances. * Look straight down the top of the beaker and you should be able to see the cross, you should stop the stopwatch when the substance becomes so cloudy that you can no longer see the cross. You should repeat this experiment for each of the concentrations that are needed varying the water and sodium Thiosulphate as you go. Diagram of experiment: My prediction If the concentration of a solution is increased there are more reactant particles per unit volume. ...read more.

Conclusion

For this to fully make sense it is necessary to recap the collision theory briefly: For a reaction to occur particles have to collide with each other. Only a small percentage of results 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. If the frequency of collisions is increased the rate of reaction will increase. However the percentage of successful collisions remains the same. An increase in the frequency of collisions can be achieved by increasing the concentration. So from the evidence I have collected from my investigation I can tell you that I had one outlier throughout my investigation but it was clear and so easily noticed and sufficiently removed. It is clear to me that the rest of my results are accurate as I have done three tests for each concentration this shows me that there was not to bigger range between results of the same category which assures me my results are accurate. Overall I feel that I have conducted a reliable and fair investigation. If I where to do this experiment again I would use a measuring cylinder as well as a burette to insure even more accuracy and sustain an experiment with no outliers. MATTHEW HUMPHREY 10D GCSE COURSEWORK ...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 report is of variable quality. Some aspects are well written but brief and there is not enough mention of the scientific theory behind the investigation. The data is of reasonable quality. There have been specific improvements suggested throughout.

Marked by teacher Cornelia Bruce 17/04/2013

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

    Rate of Reaction Chemistry Coursework

    4 star(s)

    If I don't the results would vary and would not be very good. I will control this by when I am using the magnesium strips I will only make one cut out so the surface area of the magnesium will also be the same.

  2. Marked by a teacher

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    If some particles had a larger or smaller surface area then the speed of the reaction would either be increased or decreased accordingly.

  1. Peer reviewed

    Rates of Reaction

    5 star(s)

    Using a catalyst will also increase the rate of reaction. This is because the catalyst produces an area for both reactants to stick on increasing the probability of collisions and so therefore there are more collisions increasing the rate of reaction.

  2. The aim of this coursework is to investigate the rate of reaction between sodium ...

    As the experiment continues, the more yellow sulphur precipitate is formed, thus causing the solution to become opaque. Changing the concentration of a solution affects the rate of reaction. The concentration of a solution is how strong the solution is.

  1. An Investigation of the Effect of Copper Sulphate on Catalase Activity.

    There will therefore be more oxygen produced when copper sulphate is not present. I believe this because copper sulphate will act as a non-competitive inhibiter in the reaction. I predict that the reaction will not continue when the concentration of hydrogen peroxide is increased at the end of the experiment.

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

    It should be regarded as a modification to experimental method: When mixing chemicals prior to starting the reaction, the Hydrogen peroxide should be kept separate from the acid and the Potassium Iodide. However, instead of keeping all the reactants separate and introducing more timing error in the final mixing, it

  1. Factors Affecting the Rate of Catalytic Decomposition of Hydrogen Peroxide.

    0.51 0.51 0.51 60 0.51 0.51 0.51 1.23 mol Reading 1 Reading 2 Average Time (s) Mass Lost (g) Mass Lost (g) Mass Lost (g) 5 0.15 0.16 0.16 10 0.20 0.21 0.21 15 0.28 0.27 0.28 20 0.35 0.32 0.34 25 0.45 0.41 0.43 30 0.52 0.50 0.51 35

  2. How does the concentration of HCl affect the rate of reaction with CaCO3?

    45.07 60.00 0.75 24.00 26.00 key N/a = not applicable anomalous result I got four anomalous results, three of them were very far from the averages and one of them wasn?t really very far from the average (I didn?t include the anomalies in the calculation of the averages)

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