• 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

Investigate how the concentration of hydrochloric acid affects the rate of reaction between calcium carbonate and hydrochloric acid.

Extracts from this document...

Introduction

My aim is to investigate how the concentration of hydrochloric acid affects the rate of reaction between calcium carbonate and hydrochloric acid. The word and chemical equation which I have constructed for the experiment is: Calcium + hydrochloric calcium + water + carbon Carbonate acid chloride dioxide. CaCo3 + 2HCL CaCl2 + H2 O + CO2 Reactant Product I chose this reaction because it is easy to control as the production of carbon dioxide being produced can be monitored with ease. Additionally the amount of carbon dioxide given out can me measured accurately and fairly quickly. From this equation, it is evident to us that hydrochloric acid has a large effect on the reaction. The calcium displaces the hydrogen from the hydrochloric acid which results in calcium chloride (marble) in being formed I chose concentration as the variable because of its ease in changing in comparison to the other variables - temperature, surface area, concentration and catalyst. I did not choose the variable to be temperature because it is difficult to maintain and requires precise measurements. The surface area of the marble chips would too be too difficult to measure. Additionally catalysts was not the variable I chose, because this would only give me two results - whether the rate of reaction is faster with the catalyst or whether it is faster without the catalyst. I chose not to keep the concentration constant because it is easy to change and in comparison to these three other variables I think that it will be the quickest and most accurate variable. ...read more.

Middle

* Trough - Enables carbon dioxide gas not to escape so that it can be measured. * Clamp - To securely hold the gas burette. * Gas burette - To contain the carbon dioxide gas so that it can be measured. Method * We filled up the trough and gas burette with water to the top. * Then we filled the conical flask with hydrochloric acid of the range: 20, 25 and 30 cm cubed. * Following this the gas burette was placed on a clamp and was placed facing downwards so that the open end was inside and surrounded by water. * We then placed the delivery tube in a position where it was directly beneath the gas burette and also was going through the bung. * The different sizes of chips were then weighed so that the different sizes of chips could add up to 1 gram. We found that equivalent to 1g was 1 large chip, 3 medium chips and 6 small chips. Furthermore the chips were dropped in the conical flask and the bung was immediately placed on the flask while the stopwatch was started. * After that we recorded the time taken for 50cm3 of carbon dioxide given out by stopping the timer when the burette had been filled up with carbon dioxide and therefore 50 cm3 of water had been pushed out. Results Size Of Chip Size and Quantity Of Marble Chip Time Taken For 50 cm3 Of Carbon Dioxide Gas To Be Released (mins) 1 Large chip 4.22 3 Medium chips 3.21 6 Small chips 2.23 N.B. ...read more.

Conclusion

44 48.8 46 150 8 7.3 8.5 17.5 28.5 19.6 47.2 50 47.9 160 8.8 7.9 8.8 20 30 21.6 48.4 50 170 9.5 8.5 9.3 22.5 32.7 24.3 50 180 10.1 8.9 9.7 24.7 34.5 26.4 190 11 9.6 10.7 26.4 35 28.8 200 12 9.9 10.8 27.5 36.1 30.8 210 12.7 10.7 11.6 29.6 38.1 33.1 220 12.8 11.3 12.3 31.4 41 35.2 230 14 12.5 13 33.2 43.4 37.8 240 15.2 13.7 14 34.9 45 39.8 250 15.8 14.5 15.1 36.5 47.8 42.3 260 16.5 15 15.9 39.3 49.3 44.8 270 16.8 15.7 15.9 41 49.6 46.8 280 17.5 16.4 16.3 42.5 50 49 290 17.8 16.5 17 45 50 300 18.5 16.8 17.9 48 310 18.7 17.1 18.1 50 320 19 17.8 18.5 330 19.9 18.7 18.9 340 22 20.1 20.3 350 23 20.1 21.5 360 23.3 22.5 21.9 370 23.7 22.7 22.4 380 24 23.4 22.8 390 24.7 25.6 23.2 400 26.3 28.6 25.9 410 28 28.9 26.9 420 28.4 29.1 28 430 28.8 30 29.9 440 29 31.2 30.2 450 29.6 32.1 30.9 460 31.6 33.4 31.6 470 32.9 35.1 32.5 480 35.2 36 33.9 490 35.9 36.5 35 500 36.5 37.2 35.8 510 38 38.1 36.7 520 39.1 39.5 38.1 530 40.2 40.2 39.9 540 41.7 42.1 41.6 550 43.7 44.1 43.5 560 44.9 45.3 45 570 47.1 46.9 46.2 580 48.3 48.2 47.9 590 49.5 50 49.3 600 50 50 Average Results Concentration (molar) Average time (sec) 0.5 597 1 293 2 160 3 113 4 73 GCSE Chemistry Coursework Autumn Term 2003 Ravi Dewji 11S ...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

    To investigate the effect of temperature on the rate of reaction

    4 star(s)

    70 14 12 80 17 12 90 17 12 100 19 12 110 () 12 120 () 12 ~ ~ ~ 130 - 360 () 25 Temperature at 70�C Time (secs) Vol. of gas (medium chips) Vol. of gas (large chips)

  2. Marked by a teacher

    To see how the concentration of acid, reacting with potassium carbonate, affects the rate ...

    4 star(s)

    During the different times of the week when I will be carrying out this experiment the air temperature might change rapidly because it is summer and hot days vary a lot from cooler days. To make this fair I will attempt to cool the acid down before carrying out my

  1. Peer reviewed

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

    3 star(s)

    3. Measure 25cm3 of hydrochloric acid. 4. Place a burette of water upside down in the plastic container. 5. Place marble chips inside a conical flask with a thistle tube and small funnel. 6. Connect this to the plastic container using a delivery tube.

  2. Investigating the effect of temperature on the rate of reaction between hydrochloric acid and ...

    and the time between measurements (10 seconds) the same. Apparatus. Large measuring cylinder Conical Flask Large tub Hydrochloric acid (15cm) Water Marble chips (5g) Gas tube with bung Safety glasses Stopwatch Bunson burner Tripod Gauze Heatproof mat Thermometer Small measuring cylinder Diagram. Method. Firstly I will set up the apparatus as above.

  1. Rates of Reaction

    There are three experiments I will perform these being the following: - Using a measuring cylinder to accumulate the amount of gas given off. - Mass method. - Collecting the gas in a syringe. Method 1: using a measuring cylinder in order to accumulate the amount of gas give off

  2. Rate of Reaction

    Mass 1g, CO2 vol. (ml) Mass 3g, CO2 vol. (ml) Mass 5g, CO2 vol. (ml) 0 0 0 0 10 3 13 19 20 5 24 38 30 7 33 80 40 10 39 - 50 12 49 - 60 15 79 - 70 18 95 - 80 21 100

  1. to investigate how the concentration affects the rate of the reaction

    If a lot of acid and a limited supply of magnesium are used, the hydrogen gas produced will not be as much as if plentiful magnesium and hydrochloric are used. This is because the magnesium is going to be used up by some of the acid and some of the acid will remain un -reacted 3.

  2. To investigate the factors affecting the volume of carbon dioxide produced when a carbonate ...

    o The rubber bung was replaced as quickly as possible (so that carbon dioxide didn't escape through the top of the flask). o Results of the volume of carbon dioxide were read from the measuring cylinder. o The experiment was repeated using the volumes and masses shown in the preliminary results table.

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