• 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
  11. 11
    11
  12. 12
    12
  13. 13
    13
  14. 14
    14
  15. 15
    15
  16. 16
    16
  17. 17
    17
  18. 18
    18
  19. 19
    19
  20. 20
    20

How does concentration affect the rate of reaction?

Extracts from this document...

Introduction

How does concentration affect the rate of reaction? Aim: To investigate how different concentrations of hydrochloric aci9d affect the rate of reaction on marble chip, (calcium carbonate). Background information: Different reactions take place at different rate. The measurement of the change can take place in a single unit of time; it can take seconds, minutes, hours and even days. It can be either fast or slow. Reaction rates are explained by the collision theory. The collision theory is explained by the rate of reaction. This is when reaching particles collide with each other. In order for particles to react, this depends on how often and how hard they collide. There are four main methods that are explained in terms of increasing the number of collisions so that the rate of reaction also increases between the reacting particles. These are: Temperature, concentration, surface area and a catalyst. Temperature causes particles to collide faster if the temperature is high and slower if the temperature is low. By increasing the temperature, the reactant particles are supplied with a lot of energy, they move faster and this increases the chance of more successful collisions, because the reacting particles have an increase in energy, the particles can collide hard enough to make a reaction happen. In year 9, I studied the effect of temperature on the rate of reaction. It was an experiment to investigate the reaction between thiosulphate and acid. This reaction showed that there were faster collisions at 300C than there were at 200C. At higher temperatures, ions have more kinetic energy and collide more often and more vigorously, giving them a greater chance of reacting. ...read more.

Middle

The rate of reaction of the third trial=gradient Rate of reaction of 2.0 mole of concentration = 53 = 53cm3 per minute 1 rate of reaction of 1.5 mole of concentration = 33 = 33cm3 per minute 1 rate of reaction of 1.0 mole of concentration = 13 = 13cm3 per minute 1 rate of reaction of 0.5 mole of concentration = 4 = 4cm3 per minute 1 rate of reaction of 0.1mole of concentration = 0 = 0cm3 per minute 1 Conclusion: These results show that as the concentration increases from 0.1m to 2.0m the gas produced increases from 0 to 264cm3 this indicates that as the concentration increased the rate of reaction also increased. Also based on my scientific knowledge of the collision theory I know that the higher the concentration in an acid the faster the rate of reaction, because the higher the concentration the more chances for the particles to collide more frequently and more chances for successful collisions. Apparatus: the following piece of equipment will be used to do the experiment. * Hydrochloric acid solutions- the reactants for the experiment * Marble chips/ calcium carbonate- another reactant for the experiment. * Conical flask- to put the reactant of the experiment inside. * Gas syringe, delivery tube and bung- when connected together, it will measure the volume of gas given off in the experiment, when the bung is inserted into the conical flask. * Electronic weighing scales- to measure the mass of the marble chips. * Spatula- to measure the amount of marble chips used for experiment. * Stopwatch- To time every minute until 5 minutes, so I can see how much gas is produced over a period of time. ...read more.

Conclusion

The person also checked their equipment before actually using it so there were no problems with it. If I were to repeat this experiment I would make various changes in the way I constructed myself and carry out the experiment like: * I would firstly make sure the marble chips were more accurately measured so that they are the same size. * I would wash the beakers after using them each time so that the concentrations are not diluted. * I would make sure the stop clock is started immediately as the marble chips are placed in the concentration. * I would use more concentrations so that there would be a wider summary of the experiment * My experiment would be repeated three times so I could make an average of the results, this would increase accuracy. * Keep the mass and the surface area of the marble chips the same (maybe use the powder like substance rather than different sized marble chips). * Prevent contamination-by washing the conical flask thoroughly. * The length of time in which I do the experiment could be lengthened, so I can get longer timings, this would give a better idea of the rate of reaction of each concentration. * I would use more concentrations to see how they differ form the concentrations I have used and it would give a better spread of results. I would like to further my knowledge of the topic and investigate temperature catalyst and surface on the rate of reaction on a marble chip, the thought of this is ideal but I know it is very difficult to do. I found when looking in textbooks that the graphs were demonstrated as a curve. ...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. Marked by a teacher

    In this investigation we are going to measure the rate of reaction of marble ...

    3 star(s)

    20 10 10 9 13 11 9-11 40 15 17 18 19 17 15-19 60 20 23 21 23 22 20-23 80 26 30 27 29 28 26-30 100 32 37 35 32 34 32-37 120 35 44 42 38 40 35-44 140 42 50 52 42 47 42-52 160

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

    How catalysts work: The collision theory and enthalpy profiles help us to understand how catalysts work. In a chemical reaction, existing bonds in the reactants must first stretch and break. Then new bonds can form as the reactants are converted to products.

  1. Investigate various ways of increasing the rate of a chemical reaction and evaluate which ...

    Recording the change in mass would be appropriate as carbon dioxide is quite a heavy gas. However there is only one top-pan balance available for the whole class to use. Thus we are left with the method of observing a reactant dissolve.

  2. Effect Of Substrate Concentration On The Activity Of Catalase

    Make sure to keep eyes level with ruler so as to minimise the chance of parallax error. The diameter of the cylinder remains constant due to the use of the cork borer. 6. Put the potato pieces into a boiling tube and put aside.

  1. Exothermic and endothermic reactions

    Students commonly count atoms rather than bonds. * Remember when answering chemistry questions that with double and triple bonds, the bond energies you will be given are for all the bonds shown. For example, if O = O --> 498 kJ/ mol, then the figure is for both bonds in oxygen.

  2. An Investigation: Factors That Affect The Rate Of Reaction between Calcium carbonate and Hydrochloric ...

    Time Repeat 1 (ml) Repeat 2 (ml) Repeat 3(ml) Repeat 4 (ml) Repeat 5 (ml) Averages 10 9 9 10 8 9 9 20 15 13 17 14 13 14.6 30 23 19 24 20 18 21.6 40 31 24 30 26 21 27.8 50 40 29 39 32 26

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