• 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
  14. 14
  15. 15
  16. 16

Look at two variables that affect at the speed of the reactions between Marble Chips (CaCO3) and Hydrochloric Acid (HCl).

Extracts from this document...


In this piece of coursework I am going to look at two variables that affect at the speed of the reactions between Marble Chips (CaCO3) and Hydrochloric Acid (HCl). I will use four different states of division of the marble chips. These will be: * Large chips * Medium chips * Small chips * Powder I will also vary the concentration of my Hydrochloric acid. * 2.5 Molar * 2.0 Molar * 1.5 Molar * 1.0 Molar * 0.5 Molar In any reaction a solid is needed, our solid is Marble Chips. EQUIPTMENT: * Beakers (250ml) * Measuring cylinder (50cm3) * Bungs * Thermometer (00C-110oC) * Electronic Scales (0.00g) * Weighing boats * Boiling tubes (50cm3) * Marble chips (Small, Medium and Large) * Hydrochloric acid (2.5 - 0.5 Molar) From this reaction, Carbon Dioxide is produced, and it is the collection of this gas that will measure the reaction for us. I predict that, " the more concentrated the acid, the quicker the reaction will be." Also " the larger the chips, the longer the reaction will take." I think this because a reaction occurs when particles collide. This process is based on random particle movement. ...read more.


Because of the fact that the marble chips come with a thin layer of powder on the outside, we have decided to leave the reaction for thirty seconds at the beginning before we start collecting the Carbon Dioxide. After the thirty seconds, we placed a boiling tube (50cm3) on top of the glass tube coming from the conical flask and timed to see how long it takes to fill the tube completely with the Carbon Dioxide. We will also measure the temperature of the room, because it may be carried out on different days so the temperature could have changed. This temperature change could affect our results by many seconds. I believe that my prediction that " the more concentrated the acid, the quicker the reaction will be,'' will be proven correct because stronger acids come with more severe warnings on them, thus must be more corrosive. The more corrosive an acid is the faster it should make this reaction happen. The equation is CaCO3 + 2HCl CaCl2 + H2O + CO2 Firstly we tested the different chip sizes and came up with these results. Time in Second Size of Chips Time 1 Time 2 Average Rate 1/time in seconds S 14 13 13.5 0.74 M 23 22 22.5 0.04 L 26 ...read more.


All my readings were repeated and an average was taken. If there were an anomalous result they were re-tested and changed accordingly. My equipment was kept the same the whole way thought the experiment so the only things that were changing were my variables. This means that my experiment was a fair test thus the results are as reliable as they could be. After doing my experiment and analysing my findings I can now say that there are two clear conclusions The more concentrated an acid is the faster it will react The larger the surface area of a reactant the faster the reaction will be Because of the fact that my experiment met my expectations and the exportations of basic science, I would say that my experiment has nothing that needs changing. I am very happy with the way my experiment went and with my method. However it would have been nice to get all the results done in the one day, because there could have been different factors that could potentially have affected my work, e.g. using different apparatus, the apparatus I am using may have other chemicals left in it, or there could have been a small temperature rise, that was not noticed on the thermometer, these are all small things that could affect my results in a big way. ...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

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

    3 star(s)

    9-10 160 30 13 13 9 12 9-13 180 32 13 13 10 12 10-13 200 40 16 16 12 15 12-16 220 44 16 17 15 16 15-17 240 46 16 17 16 16 16-17 260 47 18 17 17 17 17-18 280 50 18 20 18 19 18-20

  2. Exothermic and endothermic reactions

    This is why fractional distillation works. Question 6 How does the number of carbon atoms in a hydrocarbon affect its boiling point? [1 mark] The Answer The more carbon atoms it has, the higher its boiling point It would also be correct to say 'the fewer carbon atoms it has, the lower its boiling point'.

  1. Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

    This, should then double the chance of the calcium carbonate atoms and the hydrochloric acid molecules successfully colliding and reacting. Apparatus * Cone shaped conical flask * Measuring cylinder * Delivery tube * Gas syringe * Bung * Stop clock * Goggles * Mat * Balance Chemicals Required * Hydrochloric acid (1, 2, 3 and 4 molar)

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

    produced every 15 sec 15 sec Medium 9-12mm) 4g 25 ml 15 30 45 60 75 90 105 Secs 7 10 13 18 21 24 27 120 135 150 165 180 195 210 Secs 34 36 40 42 45 46 50 225 240 225 270 285 300 315 Secs 52

  1. The object of this investigation is to determine the enthalpy change for the reaction ...

    56 = 0.0245 moles Seeing as the molar mass of CaO = 56.00 ?H2 = 2520 x (1 x 0.0245) = - 102.86 kJmol-1 3) If 1.39 g of CaO then: moles of CaO = 1.39 g ? 56 = 0.0245 moles Seeing as the molar mass of CaO = 56.00 ?H2 = 2730 x (1 x 0.0245)

  2. Reactions between HCL and Marble chips.

    effects the rate of reaction, therefore I tried to find marble chips of roughly the same size. Another variable I took into account was the volume of HCl I will use; I am changing the amounts of acid in each concentration.

  1. Find out if the concentration effects the rate of reaction between CaCO3 & HCl.

    rate would be higher and the amount of CO2 would be given out more quickly. Below is an example graph as you can see that the high concentration will react: Temperature The higher the temperature the more energy each particle will have which means it will vibrate more, causing the amount of collisions to increase.

  2. How does the concentration of HCl affect the rate of reaction with CaCO3?

    * Pipette ? we used a pipette to put hydrochloric acid into the 10ml measuring cylinder because it helped us put the hydrochloric acid exactly to the 10 ml. * 0-10 ml measuring cylinder ? we used this because it eliminated any chances of us putting anything higher than ten

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