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

The aim of this coursework is to investigate how varying a factor affects the rate of reaction between Hydrochloric Acid and Calcium Carbonate (Marble).

Extracts from this document...


Ben Lloyd 11SJH Chemistry Coursework Rate of Reaction Aim The aim of this coursework is to investigate how varying a factor affects the rate of reaction between Hydrochloric Acid and Calcium Carbonate (Marble). What is a reaction? A reaction is when two particles (reactants) join to form a new product or products. What is rate? Rate is a measure of how fast or how slow something is. Rate is a measurement of the change that happens in a single unit of time, any suitable measurement can be used such as seconds, minutes, hours or even days. What is the rate of a chemical reaction? The rate of a chemical reaction is how fast the reactants react. Collision Theory For Hydrochloric acid and calcium carbonate to react the particles of each must collide with each other, the collision must have a sufficient amount of energy. The rate of reaction depends on how many successful collisions there are in a given unit of time. If there are a lot of successful collisions in a given minute, then a lot of hydrogen is produced in that minute, in other words the reaction goes quickly if the rate is high. If the concentration of the acid is increased then the reaction rate is higher and the reaction takes place quicker. There are also more successful collisions than there would be with a lower concentration. Preliminary Tests - Test 1 We put three different sizes of marble stones together with Hydrochloric Acid and measured the amount of Carbon Dioxide given off every 10 seconds. ...read more.


1.0M 2.0M 3.0M 4.0M 1 2 3 Ave 1 2 3 Ave 1 2 3 Ave 1 2 3 Ave 1 2 3 Ave 0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 10 1.0 1.0 1.0 1.0 3.0 4.0 3.0 3.3 13.0 15.0 18.0 15.3 40.0 22.0 25.0 29.0 25.0 65.0 45.0 45.0 20 1.0 1.0 1.0 1.0 6.0 7.0 5.0 6.0 25.0 30.0 35.0 30.0 80.0 40.0 48.0 56.0 50.0 110.0 85.0 81.7 30 1.0 1.0 1.0 1.0 12.0 9.0 11.0 10.7 38.0 50.0 50.0 46.0 90.0 60.0 67.0 72.3 75.0 140.0 115.0 110.0 40 1.0 1.0 1.0 1.0 18.0 15.0 17.0 16.7 50.0 57.0 65.0 57.3 110.0 78.0 86.0 91.3 100.0 ! 130.0 115.0 50 1.0 1.0 1.0 1.0 30.0 24.0 26.0 26.7 60.0 70.0 80.0 70.0 130.0 95.0 110.0 111.7 130.0 ! ! 130.0 Average 0.8 0.8 0.8 11.5 9.8 10.3 31.0 37.0 41.3 75.0 49.2 56.0 63.3 78.8 75.0 Total Average 0.8 10.6 36.4 60.1 72.4 Now I have calculated these averages the results state quite clearly that as the concentration of the Hydrochloric Acid is increased the amount of Carbon Dioxide given off in 50 seconds also increases. The reaction that takes place is: CaCO3 (s) + 2HCl(aq) --> CaCl2(aq) + H2O(l) + CO2(g) On the table of results above I have shaded two sets of results grey, the 40 & 50 seconds results. This is because the results I have gained were not gained accurately as they went off the scale of the gas-measuring cylinder. ...read more.


But disregarding the anomalies the results I do have still manage to prove my prediction. With scientific evidence to back up my prediction my results prove it. Also my graphs show that the higher the concentration the faster the reaction takes place. But even if the experiment had gathered more accurate results I would have still been brought to the same conclusion that the higher the reaction, the faster the reaction! Investigation variations This experiment went very well overall, although the factors I have discussed above did not seem to accredit the method very well. The major weakness with the method we used was the loss of gas during the process of connecting the bung to the conical flask. So the best way to solve this problem, is not to adapt the current method, but to get rid of it. I think that an alternative method of conducting this experiment would be to measure something other than the gas release. An idea is to measure the weight difference. An alternative method would be as follows: * Place a conical flask containing a fixed amount of CaCO3 in. * Take the weight of the flask and contents & add it to the weight of the fixed amount of HCl. * Keeping the conical flask on the scales add the HCl to the flask. Every 10 seconds you can take the reading of the weight as it decreases on the scales. From this I can work out the weight difference. This difference will represent the content given off as gas. From this I can derive a reaction rate. Below is an example diagram of this method: Page 1 of 1 ...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. Free essay

    Chemistry Rate of Reaction Coursework for Calcium Carbonate and Hydrochloric Acid

    other methods, like for example timing and observation, where the reliability depends on the quality of eyesight, which is never 100% accurate and will vary with different individuals. In other terms, there's less dependence on human ability, which can easily cause an error.

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

    There is a slight anomaly with one of the values, but when it came to the next reading, it matched up. There were completely anomalous results for 1.75m of hydrochloric acid, so I decided not to include it. An anomalous result An anomalous result is a result is a result that is not near the other results i.e.

  1. An Experiment To Investigate The Rate Of Reaction Between Marble Chips And Hydrochloric Acid.

    The slight anomalies could have been the result of small measurement misreadings, the slight change in the surface area of the chips or a change in room temperature but the main factors that needed to be constant were done so and this is supported by the invariability of the final results.

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

    Calcium Carbonate There is not really a danger with the calcium carbonate chips unless it is swallowed. If they are, seek medical advice straight away. Glass Equipment Nature of hazard - If glass equipment is broken, the sharp glass can cause cuts to the skin.

  1. Investigate the effect of changing the concentration of hydrochloric acid and the volume of ...

    Minutes Volume of CO2 produced (cm�) 30 0.5 10 60 1.0 55 90 1.5 97 120 2.0 135 150 2.5 173 180 3.0 203 210 3.5 235 240 4.0 263 270 4.5 285 300 5.0 310 330 5.5 330 360 6.0 347 390 6.5 362 420 7.0 375 450 7.5

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

    These other variables include: *Temperature: -temperature of the reactants are kept at room temperature. *Volume of acid: - the volume of acid is kept constant at 25cm3 *Concentration of acid: - the concentration of acid is kept constant at 1Mol/dm3.

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

    50ml will be the control for the amount of nitric acid to use and so will 5g be for the calcium carbonate. If there is too much gas produced or not enough to get a good rate of reaction I can alter these factors to change the volume of the carbon dioxide.

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

    investigating a different variable that affects the rate of reaction for example gas. to improve my experiment I will measure the gas produced but keep time as the dependent variable and the independent variable will remain the same because I will still be investigating the effect that the concentration has

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