• 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
  11. 11
    11

Rate Of Reaction

Extracts from this document...

Introduction

Investigating the rate of reaction between hydrochloric acid and marble chips. Aim. In the investigation I am going to find out the rate of reaction by measuring the amount of gas produced and weight loss in a reaction between small/large pieces of Marble Chips (Calcium Carbonate) and Hydrochloric acid per minute Calcium Carbonate + Hydrochloric Acid + Calcium Chloride + Water + Carbon Dioxide CaCO3 + 2HCl + CaCl2 + H2O + CO2 Planning The rate of reaction tells us how fast or slow a chemical takes to react. The reactant can be measured by the amount used or the amount of product gained in an amount of time. The rate of reaction is affected by 6 things: * Temperature * State of division * Catalysts * Concentration of reaction * Stirring and Shaking * Pressure. Factors Temperature: If the particles in a reaction are heated then they will gain much more kinetics energy. Low temperature particles will be less able to successfully collide and react because of their low energy. A high temperature particle would have more energy, making it move faster and making more successful collisions, this would be the rate of reaction increasing because more particles would be colliding with each other. ...read more.

Middle

* The temperature of the Hydrochloric acid must also be kept at a constant temperature due to how quickly or slowly a reaction takes place Accuracy To ensure my experiment is as accurate as possible I will measure the solutions very accurately. I will do the same when measuring the marble chips, the weighing scales I will be using are correct to 2 decimal places. I think 2 decimal places are accurate enough for this experiment as I am only using the weighing scales to measure the marble chips. I will repeat the experiment three times to make sure my average consists of a good range of results. The hydrochloric acid goes up by 0.5 molar every time so our results will not be too similar. A good range of results will be produced. If I find any anonymous results I will record them but then I will repeat the same test to see if I get a result which follows some sort of pattern. I will record my results accurately to 2 significant figures. Prediction Using my scientific knowledge I predict that as the concentration of the acid increases the rate of the reaction will accelerate causing Carbon Dioxide to be given off at a faster rate. ...read more.

Conclusion

To make the test a fairer, I could try and make the size of the chips the same, although this is almost impossible, since all marble chips are different. To make my results more accurate and reliable I could repeat the experiment a total of five times or more. The reaction could have speeded up due to human error because the conical flask could not have been washed out properly. So some acid could have been left in the beaker, making the reaction speed up. Then making my results wrong. I could try the reactions at different temperatures. I could then find the optimum temperature for the reactions to take place at. I could also try different acids such as sulphuric acid and nitric acid; I could then compare the results and ascertain which acid reacts more quickly with the marble chips. Conclusion. I have been able to successfully test the relationship between the rate of reaction between HCl and marble chips, depending on their concentration. The rate of reaction is directly proportional to the concentration, this agrees to the prediction I made. Increasing the concentration,, also meant the increase of H ions in the solution, which means that there will be more collisions between the particles. To me my results were accurate enough and the predictions I made were conclusive ...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

Here's what a teacher thought of this essay

3 star(s)

***
This is fairly basic investigation into the affect of concentration on rate of reaction. Some good diagrams should be used to support the written content. It does however need to be written with more clarity and depth. The lack of experimental data limits its reliability. Improvements have been suggested throughout.

Marked by teacher Cornelia Bruce 18/03/2013

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. Marked by a teacher

    To determine the amount of ammonia in a sample of household cleaning product, 'cloudy ...

    5 star(s)

    in 1000ml =1.153 moles ? m(NH4OH) in 1000 ml = 1.153 (14 + 4 + 16 + 1) = 40.36 g Therefore the concentration of ammonia as NH4OH in 'cloudy ammonia' is 40 g/L. This is less than the manufacturer's claim by 10 g/L.

  2. To investigate three factors that affect the rate of cooling a liquid and to ...

    Results Tables Experiment 1 No Insulation Corrugated Card Woollen Lagging 0 seconds 40 seconds 80 seconds 120 seconds 160 seconds 200 seconds 240 seconds 280 seconds 320 seconds 360 seconds 400 seconds 440 seconds 480 seconds 520 seconds 560 seconds 600 seconds 640 seconds 680 seconds 720 seconds Experiment 2

  1. The rate of reaction between magnesium and sulphuric acid.

    The closer together they are, the more often the ions collide. The more often they collide, the higher the chance of a reaction between the magnesium and the sulphuric acid. Also there are more particles in the solution that would increase the possibility that they would collide with the magnesium so the reaction rate would increase.

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

    Where it is mainly molecules, e.g. H2O (l) and it shows a weak tendency to protonate the water molecules. While a strong acid like, HCl has a value of Ka more than 102 and its position of the equilibrium mainly is to the right. Where it is mainly ions e.g.

  1. Investigating the effect of temperature on the rate of reaction between hydrochloric acid and ...

    To overcome this problem I could use a potassium carbonate tablet instead of marble chips. - The temperature of the acid would have changed after been taken off the bunson burner or out of the ice bath. This would mean the results of temperature were not accurate.

  2. Investigate the rate of diffusion of Hydrochloric Acid into Gelatine.

    There is also a curve that I have been able to draw on the graph that links all of the experiments together. When comparing the results with each other I have found that: Surface/volume Time taken to diffuse (secs) 6 834 8 276 10 216 12 175 From these results I cannot really find a definite pattern.

  1. Indirect determination of enthalpy change of decomposition of sodium hydrogen carbonate by thermochemical measurement ...

    When the reaction is complete, the temperature versus time plot can be used to establish the final baseline. These baselines are typically linear, especially if the calorimeter is well insulated, which makes the heat loss/gain relatively small. The baselines represent the temperature changes attributable to heat exchange from the surroundings.

  2. In this investigation, I try to find out whether temperature is able to affect ...

    is the temperature you want * If the temperature is too high, then pour some of the hot water out and add some cold water. If the temperature is too low, then place the beaker on the tripod and turn on the gas tap, to heat up the water by

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