• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11

Coursework: rates of reaction, strength of acid

Extracts from this document...


Coursework: rates of reaction, strength of acid I have been asked to investigate the speed of reaction of acid acting on marble chips. Aim To find out what factors effect the rate of a reaction - the reaction between marble chips and hydrochloric acid. Key factors The Quantity of marble chips used , This could increase or decrease the surface area of the marble chips. Speeding up or slowing down the reaction because with a larger surface area more of the marble is reacting with the acid. The amount of acid used, more or less acid could change the amount of time that the reaction takes. Varying the amount of acid used would alter the time for the reaction because there are more or less acid particles to react with the marble chips. More acid longer time, less acid quicker time. The strength (concentration) of the acid used, alters the amount of particles of acid in cm3, this means that as the strength increases the amount of particles increase, giving more acid particles to react with the marble chips. Increasing the acid strength will speed up the reaction but taking longer to finish because there are more acid particles to react with the marble chips. The size of the marble chips, as marble chips increase their size there is less surface area for the acid to react with. ...read more.


This is because there are more particles in the same volume so more collisions are possible every second." Preliminary work When I first set up my preliminary experiment I started with 50 ml of hydrochloric acid and one 2 g piece of calcium carbonate, measuring the amount of carbon dioxide produced. The results were to difficult to record with the equipment and to time consuming. I then decided to half the amount of hydrochloric acid and have 2g of smaller calcium carbonate to increase the surface area. I did this to speed up the reaction so that it was also easily measurable in 1 minute intervals. The method that I used for the preliminary work was almost the same system but I only used a 1000 cm3 measuring cylinder. The problem with this was that with the lower concentration acid results were hard to read. So for the real experiment I decided to use smaller measuring cylinders. Preliminary results 0.5 mol cm3 15 29 40 55 73 92 109 125 129 136 141 141 as you can se the results took to long to collect and they would not produce great graphs. Plan To test my prediction and my hypothesis I am going to put Hydrochloric acid and marble chips together and measure the amount of gas given off every minute. ...read more.


These results nearly support my prediction, that the higher the concentration the faster the reaction will take place. The later 3 sets of results support this but the first two do not this may be because the are less particles to react with the calcium carbonate . The results also support my graph shape prediction that was that the line is steeper at the start and levels of towards the end. Evaluation Looking at my graph their is one anomalous result from my 1mol results. As there is only one wrong point I have decided that it was an error in the recording of this result. I do not think that the equipment used for this experiment was accurate because the gas that we were measuring was carbon dioxide. I know that carbon dioxide is soluble with water so as it passed through the water it would have mixed and the product that was in the measuring would not be all the carbon dioxide that was given off. Taking results was not hard but a times could be confusing recording at 30 second intervals. I feel that the evidence that I collected reliable , because of the close readings and few inaccuracies. Also that the results were what the BBC Bitesize agreed with. Also when I repeated the experiment the results were similar to each other and usually only 10 difference between each other. ...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 Aqueous Chemistry 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 Aqueous Chemistry essays

  1. Marked by a teacher

    chemistry coursework

    4 star(s)

    My maximum value is 40 cm� this reaction should prove to be a fast reaction. My minimum value is 10 cm� this should prove to be a slow reaction. My preliminary results show that my maximum and minimum values will allow more than 60 seconds between my slowest and fastest result.

  2. Peer reviewed

    The Effect of Concentration on the Rate of Reaction when you React ...

    3 star(s)

    I think that this could be solved by securing the top making it air-tight and not allowing any air to get inside the system.

  1. The Rates of Reaction of Metals with Acid.

    Using this method, we can calculate the activation enthalpy of any particular reaction just by doing an experiment at several different temperatures and plotting a graph and doing the correct calculation. (As seen in the calculations section.) The Order of reaction.

  2. Rates of Reaction

    This effectively means the Activation Energy is reduced; in this case it affects an exothermic reaction (even though it does affect both types of reaction) below is a diagram to show this: I will not be using a catalyst in my experiment as they are usually used when one of

  1. Neutralisation Coursework

    * Open the burette and allow 10ml of the nitric acid into the conical flask. Swirl it around. * If the base and indicator have not turned from orange to pink the add 1ml at a time of Nitric acid.

  2. An Investigation to Measure the Rates of Reaction between Calcium Carbonate (Marble Chips) And ...

    The second time the experiment took place, the mass of calcium carbonate was kept the same but changes were made on the volume of hydrochloric acid used down to twenty centimetres cubed. With these measurements it was found that it was easier to take down the times.

  1. Investigating the effect of concentration on the rateof reaction between marble chips and Hydrochloric ...

    This is shown by the fact that with 100% concentration of acid I measured an average of 69.67cm� of carbon dioxide, the average gradually decreases apart from at 70% where it increases, but from then onwards goes steadily down.

  2. Rate of Reaction

    When this reaction occurs, we should be observing an instant reaction with the mixture visibility fizzing and releasing carbon dioxide. This means that we are able to measure the rate of reaction by the volume of CO2 emitted. Concentration - The concentration of the solution is how strong the solution is.

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