• 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

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

Extracts from this document...

Introduction

Investigating the effect of concentration on the rate of reaction between marble chips and Hydrochloric acid Section 1: Planning Introduction In this experiment I will be investigating the reaction between different concentrations of acid and marble chips. I will be measuring the speed and rate of which gas is given off. I know that the gas given off will be carbon dioxide and that the reaction will be as follows: Calcium Carbonate + Hydrochloric Acid --> Calcium Chloride + Water + Carbon Dioxide Or CaCO3 + 2HCl --> CaCl2 + H2O + CO2 On the left are the reactants. These are the chemicals that I will start off with. On the right are the products. These are what will be produced at the end of the experiment. Reactants and products are very rarely the same, as they react with one another to form other things. There will always be the same number of atoms in the products as there are in the reactants though, as none can be dragged in, or left out. Variables In this experiment I am going to change the concentration of Hydrochloric acid. I will use 2M Hydrochloric acid as 100% concentration. Here is a table to show all of the concentrations I am planning on using, and how much acid and water to put into the conical flask. It also states how strong the acid is in M. Concentration (%) Molar Hydrochloric acid (ml) Water (cm�) 100 2.0 20 0 90 1.8 18 2 80 1.6 16 4 70 1.4 14 6 60 1.2 12 8 50 1.0 10 10 I will then investigate the difference in speed of which the gas is given off, over a two minute period. I will take measurements every 10 seconds. Preliminary Work Before this experiment, I decided which size of marble chips to use from the sizes available. The different sizes of marbles chips had an average diameter of: large-1.5cm, medium-1cm, or small-0.5cm. ...read more.

Middle

In the 100% concentration test, where I used 2M Hydrochloric acid, the volume of gas had increased by about 6, 10 seconds after the last measurement. With the 90% concentration test, I have decided to ignore the first set of measurements because I feel that they are not accurate. Therefore I have remade the table as follows: A table of results for 100% concentration of hydrochloric acid, excluding the first repetetion Time (s) Repetition 2 (cm�) Repetition 3 (cm�) Average amount of gas measured (cm�) 0 0 0 0.00 10 3 7 5.00 20 7 9 8.00 30 10 12 11.00 40 15 17 16.00 50 18 21 19.50 60 21 25 23.00 70 25 29 27.00 80 28 34 31.00 90 31 38 34.50 100 34 42 38.00 110 38 45 41.50 120 41 49 45.00 I can see from this that the amount of gas measured goes up by about 4 cm� every 10 seconds. During the 80% test the gas produced increases by about 3cm� every 10 seconds. In the 70% concentration test the gas produced increases by about 4cm� every 10 seconds, this is strange because, logically it should increase by less than the 80% concentration test. By surveying the other results and the patterns that have emerged from them I would estimate that it should have increased by 2cm� every 10 seconds instead of by 4cm�. I think that this has happened because the marble chips were probably larger. This is explained in more detail under the section entitled "Anomalous Results" In the rest of the tests the rate that carbon dioxide is given off, seems to level off at about 3-4cm� every 10 seconds. Conclusion From this investigation I have learned that if an acid is concentrated it is more reactive. Being more reactive means that for instance, in this experiment, more carbon dioxide is produced and at a faster rate. ...read more.

Conclusion

Repetition Average Volume of gas Given off (cm�) Time (s) Repetition Average Volume of gas Given off (cm�) 1 2 3 1 2 3 0 0 0 0 0.00 0 0 0 0 0.00 10 4 3 7 4.67 10 4 5 5 4.67 20 8 7 7 7.33 20 7 8 7 7.33 30 10 10 10 10.00 30 10 13 11 11.33 40 13 14 13 13.33 40 13 18 16 15.67 50 17 16 17 16.67 50 16 23 20 19.67 60 18 21 20 19.67 60 20 28 23 23.67 70 23 25 23 23.67 70 23 33 26 27.33 80 25 29 27 27.00 80 26 38 30 31.33 90 28 33 30 30.33 90 29 40 36 35.00 100 30 36 34 33.33 100 31 45 40 38.67 110 32 40 37 36.33 110 34 52 44 43.33 120 35 45 40 40.00 120 39 55 47 47.00 60% Concentration 50% Concentration Time (s) Repetition Average Volume of gas Given off (cm�) Time (s) Repetition Average Volume of gas Given off (cm�) 1 2 3 1 2 3 0 0 0 0 0.00 0 0 0 0 0.00 10 6 3 6 5.00 10 3 3 3 3.00 20 8 7 7 7.33 20 5 5 5 6.00 30 11 9 8 9.33 30 8 7 8 7.67 40 16 12 12 13.33 40 10 8 9 9.00 50 20 16 15 17.00 50 13 11 10 11.33 60 25 18 20 21.00 60 16 13 13 14.00 70 28 22 23 24.33 70 20 15 15 16.67 80 33 25 26 28.00 80 22 18 17 19.00 90 36 28 30 31.33 90 25 20 20 21.67 100 40 32 32 34.67 100 27 23 22 24.00 110 43 36 36 38.33 110 30 25 25 26.67 120 46 38 40 41.33 120 34 27 27 29.33 ...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. Peer reviewed

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

    3 star(s)

    In the second diagram we can see that it is harder not to collide with particles because there are so many (highly concentrated). This shows that it would be quicker to react in a substance that has a high concentration like the second diagram than the first diagram.

  2. To investigate the rate of reaction between different concentrations of hydrochloric acid with metal ...

    right hand as well, I can then pour the acid and time it at the same time and can quickly put on the stopper without losing too much CO2. 3. Put the CaCO3 first, before the acid and use a paper funnel so that the Calcium carbonate bit does not get stuck on the side.

  1. Investigate how the concentration of 10 ml of hydrochloric acid affects the rate of ...

    If it turns out that the two results are similar it will suggest that the method that I am using produces similar results each time. I also carried out a similar experiment but the first time I used marble chips and the second time chalk dust.

  2. The effect of Acid Rain on Seed Germination.

    I can conclude that my prediction was correct and the acid rain did denature enzymes, slowing the growth of the cress down considerably. Evaluation I encountered only a few problems during my experiment which could have affected my final readings.

  1. The Rates of Reaction of Metals with Acid.

    8.66 0.115 -2.16 45 318 3.14 7.78 0.129 -2.05 50 323 3.10 7.4 0.135 -2.00 55 328 3.05 6.65 0.150 -1.89 60 333 3.00 4.95 0.202 -1.60 Phosphoric acid 0 273 3.66 226.34 0.004 -5.42 10 283 3.53 149.88 0.007 -5.01 20 293 3.41 69.97 0.014 -4.25 30 303 3.30

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    by 5. 0.000197 mol dm-3 x 5 = 0.000985 mol dm-3 Now that I know the mols of Iron (II) Ammonium Sulphate (aq) present in the titration I can work out the concentration of it. Moles = Concentration x Volume Concentration = Moles Volume Concentration = 0.000985 10 Concentration

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

    The reason for this is because the reaction is to quick to time it to every five centimetres cubed and it will not be accurate enough if to it was to be done every fifteen or twenty seconds. The reason these measurements are being used to begin with is because

  2. The Erosion of Marble

    Put the measuring cylinder with a total mass of 40 ml of solution in it on the scales along with the beaker with 30 grams of calcium carbonate in it. 7. Tare the scales. 8. Drop the Hydrochloric acid into the beaker and start the stopwatch, record how much

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