• 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
  12. 12
  13. 13

Factors Affecting the Amount of Carbon Dioxide given off when a Carbonate reacts with an acid

Extracts from this document...


FACTORS AFFECTING THE AMOUNT OF CARBON DIOXIDE GIVEN OFF WHEN A CARBONATE REACTS WITH AN ACID Introduction ACID + METAL CARBONATE --> METAL SALT + WATER + CARBON DIOXIDE When an acid reacts with a metal carbonate, a metal salt, water and carbon dioxide are produced. The amount of carbon dioxide produced depends on various factors. The aim of this experiment is to find out how much Carbon Dioxide (CO2) is given off when different masses of Calcium Carbonate (CaCO3) are reacted with Hydrochloric acid (HCl). The factors affecting the amount of CO2 produced are listed below. Variables Continuos Variables Variable Temperature Very hard to keep constant. Amount of acid As long as there is excess for all carbonate to react, it is therefore not relevant. Concentration of acid Any acid as long as there are enough H+ ions in the acid to react with carbonate. Pressure Hard to keep constant. Surface area Hard to measure surface area of powdered Calcium Carbonate. Rate of stirring Hard to keep constant and very inaccurate. Time Not relevant as rate of reaction has no effect on amount of Carbon Dioxide produced. Amount of carbonate This is the factor under investigation Discontinuous Variables Factor Type of acid All acids contain H+ ions required for reaction. Type of carbonate Some carbonates such as Sodium are soluble, therefore I will not be able to investigate. ...read more.


To keep this experiment a fair test all three times the following were kept constant: Variable Control of variable Temperature Room Temperature Type & Concentration of acid 2M Hydrochloric Acid Amount of Acid 50ml Pressure Atmospheric Type of carbonate Calcium Carbonate Rate of stirring None The following results were obtained: Experiment 1 Mass of Calcium Carbonate (g) Volume of expected Carbon Dioxide (cm3) Actual volume of Carbon Dioxide produced (cm3) 0.2 48 36 0.4 96 80 0.6 144 94 0.8 192 158 1.0 240 190 Experiment 2 Mass of Calcium Carbonate (g) Volume of expected Carbon Dioxide (cm3) Actual volume of Carbon Dioxide produced (cm3) 0.2 48 30 0.4 96 68 0.6 144 100 0.8 192 142 1.0 240 192 The results obtained above which are in bold I found to be anomalous results. In Experiment 1 -0.6g In Experiment 2 -1.0g I therefore repeated them: Repeats Mass of Calcium Carbonate (g) Volume of expected Carbon Dioxide (cm3) Actual volume of Carbon Dioxide produced (cm3) 0.6 144 98 1.0 240 188 Analysing From the results obtained I could plot the following graphs: 1) Experiment 1 - A graph to show mass of CaCO3 against amount of CO2 produced 2) Experiment 2 - A graph to show mass of CaCO3 against amount of CO2 produced 3) A graph to show mass of CaCO3 against average amount of CO2 produced with expected result All three of the graphs show that as mass of Calcium Carbonate is increased the amount of Carbon Dioxide produce increases. ...read more.


????g of MgCO3 produces 286cm3 of CO2 ????g of MgCO3 produces 228cm3 of CO2 ????g of MgCO3 produces 171cm3 of CO2 ????g of MgCO3 produces 114cm3 of CO2 ????g of MgCO3 produces 57cm3 of CO2 Therefore it can be said that for any carbonate the relationship will be exactly the same, i.e. as the mass of Carbonate is increased the amount of Carbon Dioxide produced increases directly proportionally. 2) Do the whole experiment again but using various different pieces of apparatus. I would do an experiment, which doesn't include water, therefore no gas can be lost. Apparatus required: * Syringe * Trough * Delivery Tube * Round bottomed flask * Calcium Carbonate * 2M Hydrochloric acid * Balance * 5cm Tubes Method * Set apparatus as in diagram below * Place a piece of paper on the balance and zero it * Measure out the required mass of Calcium Carbonate * Pour massed amount of Calcium Carbonate into tube * Place tube in the lip of the round bottomed flask * Connect the delivery tube to the flask * Tap gently so that the tube falls into the acid * Shake fairly gently, making sure you are holding the delivery tube so that it doesn't dislodge from under the measuring cylinder. * When all the Calcium Carbonate has reacted record the final volume of gas obtained. Diagram: ?? ?? ?? ?? ...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. To investigate the rate of reaction between different concentrations of hydrochloric acid with metal ...

    Therefore, there will be less of the reactant to react, so in turn the rate of reaction slows down with time because there is a lower concentration of the reactants now (as the reactants are used up). Therefore, the successful collisions taking place will go down, as there is a

  2. Investigate the factors, which affects how quickly Calcium carbonate reacts with hydrochloric acid.

    Figure 1 shows the effect of particle size on the rate of reaction. In fig 1a) the square represents a large lump of a substance. In figure 1B the small squares represent the same mass of a substance in smaller pieces.

  1. CalciumCarbonate + Hydrochloric Acid —> Calcium Chloride + Water + Carbon Dioxide CaCO3 +2HCl ...

    For our experiment we used 25ml of acid (All of the concentrations used the same amount) 0.25M, 0.5M, 1.0M, 1.5M, 2.0M. 'M' Means molar which is how the strength of acid is measured. The stronger the concentration of acid used will effect the amount of gas produced, the more acid used - the more gas created & visa versa.

  2. In this experiment, we aim to investigate the effect of sodium carbonate on hard ...

    - it is accurate to 0.001g (3 decimal places), so is extremely precise; * having the correct amount of soap solution (so it is made sure that the burette is used carefully and accurately); * having the correct amount of water (so the pipette must be used with great care, and not held by bulge, which renders the amount inaccurate)

  1. Investigate how the amount of heat produced by burning a fuel depends on the ...

    likely that it will reach a higher temperature than it otherwise should have, and it could possibly even begin to boil and evaporate causing inaccurate results. Rather than wait each time for the water to return to its original temperature, which would be very time-consuming, I shall change the sample of water after each reading.

  2. Investigation into how the amount of sodium carbonate used in a reaction between itself ...

    Measuring cylinders (250cm3 and 50cm3) Method SAFETY: As a safety precaution, wear goggles throughout the experiment 1) Weigh the mass of the ignition tube and record it. 2) Weigh out 0.3 grams of sodium carbonate and put it into the ignition tube 3)

  1. To investigate how concentration affects the rate of reaction in reacting Calcium Carbonate and ...

    chip works better than the powder because it is slow enough to see the increase in reaction and fast enough slowing down. Big marble chips Time in seconds and total volume of water is 50cm3 and the amount of water displaced by the carbon dioxide is in cm3 Concentration 30s 60s 90s 120s 150s 180s 210s 240s 10:40 (acid: water)

  2. AS Chemistry - Investigate the effect of sodium carbonate on hard water

    This implies that the graph will level off at the end. Method: 1. Fill a pipette with 25cm� of water using a pipette filler. 2. Empty contents of pipette into a conical flask. 3. Add 0.5g of sodium carbonate to the conical flask containing water.

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