• 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

The Reaction Between Calcium Carbonate and Hydrochloric Acid

Extracts from this document...

Introduction

The Reaction Between Calcium Carbonate and Hydrochloric Acid Planning Aim I intend to find out the effects of changing the concentration of hydrochloric acid and the surface area of calcium carbonate on the rate of reaction in the reaction below: Calcium + Hydrochloric Calcium + Water + Carbon Dioxide Carbonate Acid Chloride CaCO3 + 2HCL CaCl2 + H2O + CO2 Scientific Knowledge > Chemical reactions can take place at different speeds. > A reaction which is over in a fraction of a second is a very fast reaction i.e. it has a high rate of reaction. As the time taken for the reaction to be completed increases, the rate of reaction decreases. That is: Rate of Reaction ? 1/Time > Increasing the concentration of reactants increases the rate of reaction. > Increasing the pressure of gases increases the rate of reaction. > In both cases, there are more collisions between particles which could lead to more successful outcomes, and hence a faster reaction. > Increasing the temperature increases the rate of reaction. > Increasing the temperature increases the average speed of particles and kinetic energy. Faster moving particles result in more collisions. More collisions are successful because the particles pass the activation energy necessary for the reaction. ...read more.

Middle

Pilot Study I needed to find out what sort of range of values would be best to use to show the best range of results without being to hard to measure. I used the same method as the main experiment. I did four experiments both with different variables; my results are below: Experiment Amount of Acid/cm3 Amount of Calcium Carbonate/g Concentration Of Acid/mol/dm3 Size of particles of Calcium Carbonate Time Taken to displace 30cm3 of Water/secs. A 5 1 2 Small 55.99 B 5 5 2 Small 9.66 C 3 3 2 Large 72.04 D 1 3 2 Powder 5.44 I looked at my results. I thought that using 5cm3 of acid and 3g of calcium carbonate would work well for the first half of the experiment and again 5cm3 of acid but this time only 1g of calcium carbonate. I chose to use small chips for the first experiment and 2 molar acid for the second experiment. I chose these values because at the both extremes of the experiments the reaction would be neither to fast to measure nor take so long that time would be wasted. Apparatus i. 1x 50cm3 measuring cylinder ii. 1x 10cm3 measuring cylinder iii. ...read more.

Conclusion

I think that I measured very well in all aspects. I measured and checked everything I did. There were not any real unexpected results or anomalies to the patterns and trends discovered. The only result that was the individual replica results for was the 0.5 molar concentration experiment. The difference between replicas a and c was nearly 40 seconds. I am not too surprised with this result however because for the slower reactions the gaps between replicas tend to become larger. The longer an experiment goes on the less accurate it is likely to be. If I were to redo the experiment I would do more replicas of experiments to try to make it more accurate. I would also use a greater range of concentrations and surface areas to increase my range of results. This would make graphs more accurate and there would be more results to compare. I think that my results are strong enough to give a firm conclusion that an increase of either surface area or concentration will increase the rate of reaction. If I were to do further work I would do similar experiments using a catalyst and varying temperature to see the affects they cause on the rate of reaction. I would expect to find similar results, that they both increase the rate of reaction. Raj Purewal Chemistry SC1 2001 Page 1 of 10 ...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. Investigate how concentration of hydrochloric acid (HCL) affects its reaction with calcium carbonate (CaCO3).

    This was because I wanted to get at least eight readings. If I used the time interval of 10 seconds as I did for all of the other experiments I would have had only seven readings. Having more readings made my experiment more accurate, which is why I wanted to have at least eight readings in the first place.

  2. Prove that changing the surface area of calcium carbonate chips, either by increasing or ...

    Naturally, the more calcium carbonate used the more particles there are available to collide with the acid particles, and the faster the calcium carbonate reacts with the acid. The same goes with the amount of acid used the more particles you have, the more collisions can occur.

  1. An Experiment to show the reaction between Hydrochloric acid and Calcium Carbonate

    With a higher concentration, such as the 'medium concentration', more particles have more energy than the Activation Energy, this is shown as the area of the curve passing the line is more than with the low concentration. With the higher concentration the area of the curve across the Activation energy is a bigger proportion than the smaller proportions drawn.

  2. Investigate how changing the concentration of hydrochloric acid affects the rate of reaction between ...

    Temperature: Increased temperature gives particles more kinetic energy. This makes the particles move faster which makes them more likely to collide. This changes the rate of a reaction. In my experiment temperature will not really be a factor. However, if I collect my results on two or three different days, then one day could be hotter than the others.

  1. Investigating How the Concentraton of Hydrochloric Acid Affects the Rate of Reaction With Calcium ...

    than an acid with a weaker. As the reaction carries on the gradient of the graph is decreased as there is more products in the solution that being water in this case which is almost hampering the reaction from continuing at the same rate.

  2. Investigation of the reaction between Hydrochloric Acid and Calcium Carbonate chips

    This makes the chance of a collision more likely. More reactions means a higher rate of reaction and the solid will be dissolved by the acid quickly. Which variable and why? I am going to investigate how the concentration of the acids changes the rate of reaction. I have chosen to do this because it is interesting yet simple and I believe the other variable are harder to investigate.

  1. Investigation into Varying Concentration of Hydrochloric Acid Effects its Rate Of Reaction with Calcium ...

    We could of changed the temperature of the acid but this would have been hard to do repeat experiments as you couldn't get the same temperature each time. We could have also changed the surface area of the calcium carbonate but the results where too hard to read, as the rate of reaction was too fast.

  2. Investigating the rate of reaction between hydrochloric acid and calcium carbonate

    quickly and more evidently whereas afterwards there was still solid that appeared at the bottom of the solution taking an overall time of 340 seconds to end. Not only can we tell the rate of reaction by observing the time taken for the whole reaction to be neutralized but I

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