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

Investigating the rate of reaction of hydrochloric acid with calcium carbonate

Extracts from this document...

Introduction

Chemistry Coursework Douglas Dixon Investigating the rate of reaction of hydrochloric acid with calcium carbonate Introduction We are going to investigate the rate of the reaction between hydrochloric acid and calcium carbonate. Our task is to "to investigate how varying the concentration of acid will effect the rate of the reaction between hydrochloric acid and marble / limestone." The equation of the reaction is: Calcium carbonate + Hydrochloric acid --> Calcium + Water + Carbon chloride dioxide CaCO3 (s) + 2HCl (aq) --> Ca Cl2 (aq) + H2O (l) + CO2 (g). Background Knowledge Rate is a measure of how fast or slow something is. For example, Silver Chloride precipitating is a very fast reaction while Concrete setting may take a couple of days to harden. Rate is a measure of the change that happens in a single unit of time. Any suitable unit of time can be used - a second, a minute, an hour or even a day. To find the rate of reaction, you should measure: The amount of reactant used up per unit of time or the amount of a product produced per unit of time. Reactions are important in everyday life. Carmakers would not be very profitable if the car they made only lasted a few days or hours before oxidizing with the air. ...read more.

Middle

The thinner you cut the slices, the more slices you get and so the more butter and jam you can put on them. This is "Bread and Butter Theory". By chewing your food you increase the surface area so that digestion can go faster. 4. Amount of acid or marble-It is important to get the right amount of marble and acid if one them is in too small amount then there will be an incomplete reaction. Keeping this in mind I have decided to use excess quantities of acid to insure there is a complete reaction. *Note: Another variable would be the use of a catalyst. The reaction will be faster but the catalyst will not be used up during the reaction. When the activation rate is lower not much energy is needed to make the reaction successful. But we are not going to use a catalyst in this experiment so it is not a factor needed to be considered. Controlled variable: I will test change the concentration of the experiment to see if this affects Prediction I predict that if the concentration of the HCl is doubled then the experiment will happen twice as fast. This is because twice as many HCl particles will be present than previously and there will be twice as much chance of the calcium carbonate chips colliding with the concentrated hydrochloric acid. ...read more.

Conclusion

complete Verdict 2.00 mol/dm3 2.00g 3.59 seconds Much too fast 2.00 mol/dm3 1.00g 7.12 seconds Much too fast 1.00 mol/dm3 1.00g 25.66 seconds Too fast 1.00 mol/dm3 0.50g 67.77 seconds Still relatively fast, but will work for the highest concentration. 0.50 mol/dm3 0.50g 83.00 seconds Good length 0.01 mol/dm3 0.50g Over 2 minutes Too slow The results show the reaction went too quickly or too slowly to record results. It also was difficult to read the results as the measuring cylinder needed to be turned upside down in the experiment meaning the label we read from to record results were also upside down. For the experiment we re-decided that the mass of the marble to be only 0.5g but to keep the marble in its powdered form. Powdered marble is easier to measuring out than larger lumps that would be varied masses. Both the form and the mass of marble would remain a constant variable throughout the experiment. New improvements to the apparatus now meant that we would use a gas syringe instead of the measuring cylinder that was harder to use. Are input variable (the acid) would be measured from 0.2 mols to 1 mol at 0.2 mol intervals. Experiment The apparatus we are using are similar to the experiment using magnesium ribbon. We found this to be the most success apparatus to record accurate results with so far. The apparatus were as follows ...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

    The Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Calcium ...

    3 star(s)

    This prediction has been created, because according to the collision theory particales will only react succesfully IF they have enough energy to to collide with one another. This means that a high conentration level in a solution gives more particals in the reaction to react with and collide with one

  2. Marked by a teacher

    What affects the rate of a reaction? The reaction I will be investigating is ...

    3 star(s)

    CaCO3 + 2HCl --> 1.0 M Moles = Concentration x volume of HCl = 1 x 20/1000 = 0.02 Moles of HCl = 0.02 Moles of CaCO3 = 1/2 x 0.02 = 0.01 Mass of CaCO3 = 0.01 x 100 = 1g From this I was able to conclude that

  1. Chemistry Cwk Rates of reaction: Investigating One Factor Which Affects How Fast Calcium Carbonate ...

    These results are terrible to calculate the rate of reaction as there are only two values. Changes that can be made to this are that smaller time intervals could be incorporated or smaller quantities of the two reactants could be used.

  2. Measuring the Rate of Reaction between Hydrochloric Acid and Calcium Carbonate

    14 30 23 27 24 25 40 40 38 34 37 50 47 43 45 45 60 56 54 60 57 70 59 58 65 61 80 65 68 70 68 90 73 77 76 75 100 90 89 84 88 110 97 93 94 95 120 100 98 97

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

    Hydrochloric Acid Nature of hazard - Higher molar acid may cause irritation to the skin. Blindness can actually occur if it comes into contact with your eyes. Lower molar acid may still harm the eyes or a cut if it drops on it.

  2. Investigation into the digestion of milk by Trypsin.

    put a dotted line on the graph to show, (according to the trend that the line of best fit forms), where I believe the maximum temperature at which the enzymes will not react due to their dormant state is. From the graph it is clear that the fastest rate of

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

    at the moment I am satisfied with my preliminary experiment because the data seems to be reliable and I was able to point out any factors that could be changed by evaluating the procedures. Actual Experiment For my Actual improved experiment there were two methods I could've used for an

  2. An Investigation: Factors That Affect The Rate Of Reaction between Calcium carbonate and Hydrochloric ...

    Then we would record the results in the table and repeat the same experiment 5 times to make the results precise and reliable. Results for surface area. We first started off with calcium carbonate powder (1.5g)with hydrochloric acid (30ml) but the reaction took place within 5 seconds and immediately reacted.

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