• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10

Rates of reaction throughout the year

Extracts from this document...


Corroding Statue I am trying to find out if a statue made of magnesium corrodes at different rates through out the year. Scientific Knowledge: Some scientific knowledge, like the collision theory and information and equations on the origin of acid rain, will help me in my investigation. Useful definitions: Activation energy: this is the minimum energy that two particles must posses for a reaction to occur when they collide. Catalyst: A catalyst speeds up a reaction by reducing the activation energy. Collision Theory: For a reaction to occur, the reactant particles must collide with each other and with enough energy (activation energy). How different conditions affect the rate of reaction: Temperature- Low temperature High temperature -Low temperature- few collisions, low rate of reaction. -High temperature- more collisions, high rate of reaction. . Concentration- Low concentration High concentration -Low concentration: particles far apart, few collisions, low rate of reaction. -High concentration: particles more crowed more collisions high rate of reaction Surface area- Low surface area ............ High surface area -Increase in surface area, increases the rate of reaction. -Smaller particles have a larger surface area than larger molecules. Catalyst- A catalyst is a substance which speeds up a reaction by lowering the activation energy but is chemically unchanged at the end of the reaction. ...read more.


I will repeat this 4 more times but I dilute the acid with more water every time. The second time there will be 40cm� of acid and 10cm� of water, the third time there will be 30cm� of acid and 20cm� of water, recording my results each time. I will continue this until there is 40cm� of water and 10cm� of acid in the beaker. I will insert my results into a table, and make graphs of my data. I will conduct the experiment a second time to get the most accurate results I can Safety Precautions: * I will wear an apron at all times. * I will wear goggles at all times. * Any acid spills that might happen, I will clean it up with a damp cloth. * Chairs and school bags will be tucked in under the table. Possible sources of error: 1. Magnesium strip not being placed flat on the surface of the acid. 2. Volumes incorrect. 3. Time not started correctly. Obtaining evidence: What I did: First, I measured out a 5cm strip of magnesium. Next I measured out 50cm3 of sulphuric acid, using a measuring cylinder, and poured the sulphuric acid into a beaker. Next I took a 5cm magnesium strip, making sure the strip was flat, and dropped it in the all acid solution. ...read more.


If I used the gas syringe my graph would look like this: Diagram of gas syringe: Improvements: If I did the experiment again the improvements I would make would be: * I would measure out the water and sulphuric acid to a greater degree of accuracy. * I would make sure the magnesium strip was completely flat when dropping it into the solution. * I would be more accurate on my timing. * I would repeat my experiment again to get more accurate results. Were my results accurate enough? : Yes, I think my results were accurate because the shapes of my graphs were what I predicted. The rate vs. concentration was proportional on my graph, and time vs. concentration was inversely proportional on my graph. Results that did not fit the pattern: In my experiment I got a few results that did not fit the predicted pattern. This may be because of a few things: * The beaker was not rinsed out properly, so that affected the concentration. * The magnesium was not cleaned properly. * There may have been temperature fluctuations. Are my results good enough to convince other people? : Yes, I think they are because the results fitted exactly with my predictions, they are straight forward and easy to read, the results and method were based on sound scientific knowledge, the results are reproducible and the there are valid reasons why the magnesium statue corroded. ?? ?? ?? ?? 1 Adam Brown 11L - Chemistry coursework ...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

Here's what a teacher thought of this essay

3 star(s)

3 Stars
This laboratory investigation into magnesium corrosion begins well with a well researched introduction. The main section of the report is too brief and does miss key elements essential to any good laboratory report including a labelled method diagram and step wise easy to follow instructions. More care also needs to be taken when evaluating the results simply stating that the results supported the prediction is insufficient, more links need to be made between the result and the science behind both corrosion and the reaction between a metal and an acid. Improvements have been suggested throughout the text.

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 Patterns of Behaviour essays

  1. Marked by a teacher

    Rate of Reaction Chemistry Coursework

    4 star(s)

    We also used preliminary to test if all the equipment that we choose to use was working well and that we would be able to use it successfully when performing our experiment. Method Reaction Red- Reactants Blue- Products Hydrochloric Acid + Magnesium Magnesium Chloride + Hydrogen HCl + Mg MgCl

  2. Marked by a teacher

    The effect of concentration on the rate of reaction of Magnesium with Sulphuric Acid.

    3 star(s)

    For this experiment I am going to find the rate of the reaction by measuring the amount of hydrogen gas produced per 180seconds. The rates of most reactions can be related to the concentrations on individual reactants by an equation: Rate = k [X]n This expression, in which X is

  1. Peer reviewed

    Rates of Reaction

    5 star(s)

    - so more collisions will be successful and the reaction will be faster. It basically provides a surface for the molecules to attach to, thereby increasing their chances of bumping into each other. So above are the four ways of increasing the rate of reaction.

  2. The effects of caffeine on reaction time

    437 332 105 13 477 360 117 14 555 480 75 15 400 250 150 16 460 360 100 17 565 320 245 18 420 309 111 19 405 190 215 20 350 231 119 Anomalous results: There are some anomalous results where the difference in reaction time is very less as in person 2-23seconds, and person 6-11seconds.

  1. Concentration and rates of reaction - "Disappearing cross" experiment.

    Possible reasons for the anomalous results could have been down to either poor observation skills, or not rinsing the conical flask out properly. There could have been more water in there than anticipated, therefore making the solution less concentrated than it should have been.

  2. An Investigation of the Effect of Copper Sulphate on Catalase Activity.

    Repeat this process twice. If no oxygen is produced after hydrogen peroxide is added for the second time then copper sulphate must be an irreversible inhibitor. It is important to use a burette as it will measure to the nearest mm3 how much oxygen is produced.

  1. How does changing the concentration of the Hydrochloric acid affect it reactions with Magnesium?

    length 3cm of magnesium ribbon, so it totals 30cm of magnesium however the surface area is increased/reduced to help the reaction. 3) After you have measured the substances for solution 1, get the stopwatch ready and place the magnesium ribbon in the colinder.

  2. A-Level Investigation - Rates of Reaction – The Iodine Clock

    For example: Figure 1.1 Zeroth Order First Order Second Order Prediction of Rate Equation For the Iodine Clock Reaction I predict that the reaction will be; Zero order with respect to [H+] First order with respect to [H2O2] First order with respect to [I-] Therefore I predict that the overall

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