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

In this Investigation, I am going to investigate the effects of concentration on the rates of reaction between magnesium and hydrochloric acid.

Extracts from this document...


Introduction: In this Investigation, I am going to investigate the effects of concentration on the rates of reaction between magnesium and hydrochloric acid. There are four factors that affect the rate of reaction, temperature, concentration, surface area and catalyst. For any reaction to occur the reactants must collide hard enough to break the bonds in the reactants, new bonds are also formed when the reactants collide with each other successfully, and the new bonds that are formed make new products. If the temperature is increased then the reaction will speed up because the heat makes the particles move faster, this makes the average kinetic (movement) energy of the particles to increase. The kinetic (movement) energy of the particles increase and become greater then the activation energy. The particles collide with each other so hard that it causes bonds to break and new ones are formed. In the same volume, there are fourteen particles, the slower they move, the lower the temperature and the faster they move, the harder they collide. ...read more.


Therefore, collisions will take place more often between particles of the crushed solids and the particles of the liquid reactants, this results to more successful collisions that lead to the reaction being faster. A catalyst speeds up the rate of reaction of a chemical reaction, because the catalyst provides another way for the reaction to take place with a lower activation energy. Therefore there will be more successful collisions at any temperature because more of the molecules will have energy greater than the activation energy. Aim: to determine if the concentration of hydrochloric acid affects the speed of the reaction of calcium carbonate with hydrochloric acid. Word equation for this reaction: Calcium carbonate + Hydrochloric acid --> Calcium Chloride + Water + Carbon Dioxide CaC03(s) + 2HCl(aq) --> CaCl2(aq) + H20(l) + C02(g) Reactants Products Preliminary method: The method I used to track the rate of reaction was by using the "Evolution of gas" method, I chose this method because the results were easier to take down and I had the right equipment for this method. ...read more.


* The mass of Calcium Carbonate Analysis & Conclusion: My results show that as the concentration increased, the volume of which carbon dioxide was produced increased rapidly. When the Concentration was 0.5M, at 50 seconds, 15cm3 of volume was produced, whereas when the Concentration was 1.0M, at 50 seconds it was 55cm3, and when the Concentration was 1.5M, at 50 seconds it was 75cm3. When the concentration was 2.0M, at 50 seconds the volume of carbon dioxide produced decreased, at 50 seconds, the volume was 53cm3. The results went as I expected except at 2.0M when the volume of carbon dioxide produced decreased when I expected it to increase. Evaluation: I think that the anomalous results may have arisen by inaccuracies. Calcium Carbonate was not measured out to the exact amount need or not enough acid. Also, the conical might have been shaken during the experiment which has an effect on the reading. Time intervals were to long, for example 60 seconds interval. Rinsing out the Conical flask properly after each experiment is vital as chemicals from the previous experiment may have an effect on the reading/result of the experiment. ...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 project I am going to investigate rates of reaction of an indigestion ...

    3 star(s)

    I measured it at 30-second intervals to see how long the reaction took. My results were: Time (seconds) Mass (g) 0 109.51 30 109.44 60 109.37 90 109.32 120 109.31 150 109.30 180 109.30 I felt there was not a sufficient difference in mass (only 0.21g)

  2. Marked by a teacher

    The effects of concentration on reaction rates

    3 star(s)

    * 6 x 10ml of hydrochloric acid - each having a concentration of 0.1M, 0.2M, 0.5M, 1M, 2M or 4M. * 10ml measuring cylinder to measure amounts of acid used. * 6 test tubes. * Test tube rack. * Stopwatch.

  1. An Investigation into how concentration affects the rate of reaction between magnesium and hydrochloric ...

    Experiment 1 Concentration of Acid(Moles) Initial Temperature(Degrees) Final Temperature(Degrees) Temperature Difference(Degrees) 0.25 15 26 11 0.5 15 59 44 0.75 17 40.5 23.5 1 17 43 26 1.25 17 48 31 1.5 18 51 33 1.75 18 52 34 2 16 51.5 35.5 Experiment 2 (Supplementary) Concentration of Acid(Moles)

  2. Investigating the factors that affect the rates of reaction between magnesium and hydrochloric acid

    Measure 10cm of Mg and put it into the flask and quickly put the bung into the flask. Start the stopwatch immediately and then take the reading on the syringe every 30 seconds. Do this until the reaction stops. Then, repeat the experiment using more and more concentrated HCL.

  1. Investigating making Epsom salts by varying the rates of reaction.

    The other reason to why we did not have time to do the last experiment was due to we forgot on several occasions to wash out the conical flask and we often remembered after we added the acid inside and the magnesium, so we had to take it out spill

  2. Concentration of Acid Rates of Reaction Investigation

    The use of a catalyst lowers this minimum energy so the reaction will happen quicker. Concentration of acid If an acid is used in a reaction, its concentration can affect the rate. At a high concentration, there are more acid particles in a certain volume.

  1. The Effects of Hydrochloric Acid on Rates of Reaction.

    The products that are formed during this reaction are hydrogen gas and magnesium chloride. The formula equation for this experiment is: Mg + 2HCl (r) MgCl2 + H2 Magnesium + Hydrochloric acid ? Magnesium Chloride + Hydrogen ( s )

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

    We measured this by using an electronic balance and we used 2M of hydrochloric acid of a volume of 30ml by using a measuring cylinder which allowed us to measure the volume accurately. For the third experiment we used large calcium chips with the mass of 1.5g.

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