• 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

An investigation into how changing one variable influences the rate of reaction between marble chips and dilute hydrochloric acid.

Extracts from this document...


Chemistry coursework Planning Section This experiment is an investigation into how changing one variable influences the rate of reaction between marble chips and dilute hydrochloric acid. When dilute hydrochloric acid reacts with marble chips the following reaction occurs: CaCO3 + 2HCl = CaCl2 + H2O + CO2 List of variables which could affect the rate. * Surface area: The bigger the surface area of the marble chips means that there will be more CaCO3 particles which means there will be a higher rate of reaction because there is a higher possibility of acid particles hitting the marble chips. * Temperature: The higher the temperature the bigger the reaction takes will be when the temperature is higher the acid particles have more energy which means they hit the marble chips harder, therefore the reaction takes place faster. * Concentration: The higher the concentration of Hydrochloric acid the higher the rate of reaction will be because there are more acid particles, which means there is a higher possibility that there will be collisions between the hydrochloric acid particles and marble chips. A list of variables which I will attempt to keep the same. * Temperature: I will try to keep this constant by having a thermometer in my solution and always checking that it is at room temperature. ...read more.


Method. * Set up apparatus as shown below. * Weigh 5 grams of marble chips and put them in the conical flask. * Make the concentration of HCl and H20, first it will be 50cm3 of HCl and 0cm3 of H20. * Start the stopwatch. * Wait until 30 seconds has passed then pour in the solution and time how long it takes for 20cm3 of water to be displaced. * Take 30 seconds off the time to get the true time. * Fill in table. * Repeat the experiment three times using the same concentration. * After you have done that repeat the experiment using the concentrations: 40cm3 HCl + 10cm3 H20 then 30cm3 HCl + 20cm3 H20 then 20cm3 HCl + 30cm3 H20 then 10cm3 HCl + 40cm3 H20. The apparatus I need are as follows: * 1 50cm3 measuring cylinders * 1 Tub * 1 Stopwatch * 1 Conical Flask * 1 Bung * 1 Top pan balance * 1 Burette Accuracy: To obtain the up most amount of accuracy I will get down to the same level as the burette while measuring the quantities of chemicals used. This will stop any misreads because of the angle I am standing at. I will make sure that my HCl and my H2O does not get contaminated. ...read more.


Evaluation The evidence I collected I believe was quite accurate. I only had one anomaly which was in test 2 of the concentration: HCl: 40 + H20: 10. This probably occurred because the bung was not secure in the conical flask which may have led to contamination or leakages of gas. In my opinion there were flaws in the method of testing. There were too many things to do at the same time for example, I had to pour acid into the conical flask and secure the bung and I also had to put the end of the tube under the measuring cylinder. To overcome this flaw I believe it would be best to do the test in a group of at least five so the tasks can be shared. Another flaw was the difficulty of getting a precise reading for the displacement of gas, to combat this next time I will use a stand which would hold the measuring cylinder in place. The evidence is sufficient to support my conclusion. There was only one anomaly, this occurred because of the reasons above. Further work I could do to provide additional relevant evidence could be doing more concentrations like 0.5, 1.0, 1.5 molar etc. because it would be interesting to see if the results also follow the trend of my graph. Also I might obtain evidence to see how catalysts, temperature, or surface area affect the rate of reaction. Craig Smith 10TER 10L 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. Marked by a teacher

    Marble Chips and Hydrochloric Acid.

    4 star(s)

    I believe that our results were probably most affected by the size of the marble chips that we used. Although they were labelled 'medium' sized and we measured as near as possible to the mass of 5g, a small range of particle sizes could have been, and were present.

  2. Marked by a teacher

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

    3 star(s)

    0 0 20 8 3 2 1 2 1-3 40 10 3 4 3 3 3-4 60 11 5 4 5 5 4-5 80 14 5 6 7 6 5-7 100 15 7 9 8 8 7-9 120 19 7 9 9 8 7-9 140 24 10 9 9 9

  1. Free essay

    Close Your Eyes

    "What...like a complete retard?" I asked and everyone laughed. "Heeey, I'm not that bad" Tom said moving his head of my shoulder and folding his arms. "No of course your not" I said "Now, anyone want a drink?" <BR?< o:p> *Carrie* Dougie had offered to buy drinks and we all accepted.

  2. Investigating the reaction between Marble Chips and Hydrochloric Acid.

    The surface area of the marble chips however were very varied (diameters of between 2mm and 4mm), therefore meaning that the variable of surface area was also controlling the results that I obtained from the experiment in addition to that of concentration.

  1. To investigate the factors which affect the rate of reaction between marble chips and ...

    that if the surface area is increased, the rate of reaction will increase at a proportional rate. I have chosen this variable because:- The temperature will be very hard to control, as it never remains constant and difficult to get the exactly right temperature.

  2. An Experiment To Investigate The Rate Of Reaction Between Marble Chips And Hydrochloric Acid.

    However, this experiment is to find out if the concentration of hydrochloric acid affects the reaction. This means that all the other ways to speed up a reaction will not be used in order to prove that it is the concentration that causes any changes.

  1. Investigation of the reaction between marble chips &amp;amp; dilute hydrochloric acid.

    Here is what apparatus I will use. Equipment Conical Flask Measuring Cylinder Stopwatch Delivery tube Plastic box Electric balance (weighing machine) I will wear goggles due to the fact that I am handling acid. I am going to test five different concentration of hydrochloric acid, going to take five readings for each acid for my preliminary experiment

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

    When I increase the concentration of calcium carbonate to 1m the amount of carbon dioxide is being increased rapidly between 10 seconds of a volume of 5ml and 120 seconds of a volume of 71ml at a range of 66.

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