• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

An investigation to compare the % by mass of calcium carbonate in a variety of common rocks.

Extracts from this document...


An investigation to compare the ? by mass of calcium carbonate in a variety of common rocks. My aim is to accurately determine the ? by mass of calcium carbonate in 4 common rocks. To do this I will need to investigate the physical and chemical properties of suitable rocks and decide upon an appropriate practical procedure to achieve satisfactory results. I will also need to consider practicality, as resources are limited. All rocks are made of minerals and these minerals have certain predictable properties. Rocks can be dissolved, diluted, decimated, decomposed, etc. However I think the most appropriate process would either be a titration involving hydrochloric acid (CaCo3(s) + 2HCl(l) ? CaCl2(aq) + CO2(g) + H2O(l)) or a thermal decomposition (CaCo3(s) ?Heat? CaO(s) + CO2(g)). The titration would involve a reaction between the rock and hydrochloric acid, which will give off carbon dioxide, which would be measured and used to calculate the results. The thermal decomposition would 'break down' the calcium carbonate into Calcium oxide and carbon dioxide, either of which could be measured and used to calculate the mass required. ...read more.


Heat with a roaring blue flame, recording the weight every 5 minutes until there is no mass loss 5. Take the final weight from the initial weight to give the mass loss 6. Repeat as above for magnesium carbonate Results: CaCO3 (in g) MgCO3 (in g) 10 mins 10.921 13.186 15 mins 10.876 13.178 20 mins 10.806 13.172 25 mins 10.761 13.172 Crucible mass 8.183 12.765 Initial mass 11.184 13.769 Total mass loss 0.432 0.597 The calcium carbonate had not finished decomposing but it is clear to see that the magnesium had ceased to decompose after losing nearly 0.6g. This test re-enforces the evidence for a thermal decomposition being the best option as it clearly distinguishes between the two carbonates. So from this it can be acknowledged that magnesium carbonate will decompose before calcium carbonate. Test 2- this test will demonstrate how easily calcium carbonate will decompose compared to magnesium carbonate. 1. Weigh crucible 2. Add calcium carbonate and re-weigh 3. Heat over a gentle blue flame for 5 minutes 4. ...read more.


to give the mass loss of calcium carbonate 10. Using information from previously stated sources that for every CO2 molecule given off, there remains one molecule of CaO and for every mole of CO2 given off, there is one mole of CaCO3. 11. Subtract the mass of CaO remaining from the mass of the other remaining substances and add it to the mass of CO2 lost. This will give the mass of CaCO3 that was in the rock 12. Work out the percentage of CaCO3 that was originally in the rock Calculations: In order to demonstrate the scientific calculation, I will use some 'convenient' numbers. Example results: Total mass of sample = 50g Mass loss of CO2 = 5g (Number of moles = mass / mr) (Mass = number of moles x mr) Example calculation: Moles of CO2 = mass CO2 / mr CO2 = 5 / (12+(16x2)) = 0.113636 mol dm-3 Moles of CO2 = moles of CaCO3 Therefore moles CaCO3 = 0.113636 mol dm-3 Mass CaCO3 = moles CaCO3 x mr CaCO3 = 0.113636 x (40+12+(16x3)) = 11.3636g Therefore ? by mass of CaCO3 = (Mass CaCO3 / total mass of rock sample) x 100 = (11.3636/50) x 100 = 22. ...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 Classifying Materials 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 Classifying Materials essays

  1. Peer reviewed

    Rate of reaction between Calcium Carbonate and Hydrochloric Acid

    4 star(s)

    Put piece of paper on digital balance and (re-zero) it. 7) Measure 2g of marble chips ( picking randomly by eye- approximately of same sizes) 8) Pour 50ml of 0.2 molar HCL into plastic measuring cylinder. 9) Pour the 50ml HCL from the measuring cylinder into conical flask. 10)

  2. The rates of reaction between CaCO3 and HCL

    procured will be the same for each sample as the amount of reactions and the duration of the experiment remains constant no more or less heat can be produced so this will not affect the data. * Surface Area, the form of limestone used is a powered form this increases

  1. Making magnisium carbonate (MgCO3)

    In MgCO3 the mg atom loses the two 2 electrons on its outer shell making it Mg2+ while the CO3 gains 2 electrons to make CO3 2- FAIR TEST * To the risk of contamination I will clean the apparatus before use * I will allow time for the reaction

  2. To investigate the thermal decomposition of copper carbonate and try to prove that the ...

    0.4 14.66 15.06 15.46 15.32 0.26 0.14 35% 0.6 13.96 14.56 15.16 14.97 0.41 0.19 31.6% 0.8 12.84 13.64 14.44 14.15 0.51 0.29 36.2% 1.0 13.54 14.54 15.55 15.20 0.66 0.34 34% Conclusion: To make an accurate conclusion I have made an average table so that I am able to

  1. Calcium carbonate reacts with dilute hydrochloric acid according to the equation below

    Mass (g) Change in mass (g) Mass (g) Change in mass (g) Mass (g) Change in mass (g) 0 60.93 0.00 59.28 0.00 58.42 0.00 15 60.80 0.13 59.14 0.14 58.31 0.11 30 60.65 0.28 58.96 0.32 58.21 0.21 45 60.47 0.46 58.81 0.47 58.07 0.35 60 60.31 0.62 58.66 0.62 57.95 0.47 75 60.15 0.78

  2. Rate of reaction of hydrochloric acid on magnesium.

    because it is highly transparent which is very easy to see through where as plastic is not. * The device to measure how much hydrogen (gas) is produce must be constant the whole experiment because the same accuracy needs to be applied to monitor the gas given off.

  1. Our experiment consisted of two samples of water containing unknown substances, and our objective ...

    - Add hydrochloric acid and barium sulphate to the solution and if a white precipitate forms immediately, then the anion is a sulphate. An ionic equation would be Halide ions - Acidify the solution of chloride, bromide or iodide by adding nitric acid.

  2. Ions - a qualitative analysis on our chemicals by flame testing.

    The following equipment and materials were gathered: * Chemicals: i. Copper-An element found on the periodic table as Cu its atomic number is 29 and has an atomic weight of 63.546 and is classed as a Coinage metal. It is a malleable and a good conductor of heat and electricity.

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