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

Chemistry - Rate of Reaction

Extracts from this document...


Chemistry Science Coursework Investigating the effect of changing concentration on the rate of a reaction. Introduction Magnesium is a highly reactive metal, in the reactivity series. What I will be investigating in this experiment is to try and find out whether or not there is any correlation between the concentration of the Hydrochloric acid and the rate of reaction. I will be using 5 different concentrations of the acid. A 2cm strip of magnesium will be dropped into the acid solution and the time it takes for the strip to completely disappear will be recorded using a stopwatch. Because this reaction is between an acid and a metal then there will be two main products formed which will be a salt and a gas. In this case the salt produced is Magnesium Chloride and the gas produced is hydrogen. Acid + Metal Salt + Gas Hydrochloric + Magnesium Magnesium Chloride + Hydrogen Acid This reaction is an Exothermic Reaction. This means that heat is produced whilst the reaction is taking place. This is all because when a chemical reaction takes place chemical bonds are broken and new ones are formed. ...read more.


2. Cut the magnesium strip in 2cm sections using the ruler, 15 strips should be cut altogether. 3. Measure 50ml Hydrochloric acid using a 50ml measuring cylinder and pour accurately each time into the 100ml beaker. This is 100% concentration of the acid. 4. Drop the magnesium strip (2cm) into the solution while starting the stopwatch simultaneously as the magnesium falls into the solution. 5. When the magnesium strip has completely disappeared stop the watch 6. Record the time taken for the Magnesium strip to disappear. 7. Repeat steps 2 to 6 changing the concentration of the acid using the table below %Concentration Volume of Acid Volume of Water 100% 50ml 0ml 80% 40ml 10ml 60% 30ml 20ml 40% 20ml 30ml 20% 10ml 40ml 8. repeat each experiment 3 times for each concentration to check the reliability of results Safety- Goggles must be warn, because the hydrochloric acid us harmful and must also be handled very carefully. Work in a safe manner. Fair testing * Used the same volume f hydrochloric acid for each reaction (50 ml). * Used same length of magnesium strip (2cm) ...read more.


fluctuation in the room temperature. The test could have been carried out using an alternative method, whereby the volume of the hydrogen gas produced could be measured against the time taken at different concentrations. Some variables could not be controlled due to the environment the test was carried out in e.g. temperature. Furthermore human error could have also affected the test e.g. measuring the solution or timing the reaction. To improve my experiment I could have used more ranges of concentrations e.g. 5%, 10%, 30% etc. I also could have investigated different sizes of magnesium or different surface areas. I could have also used different quantities of the solutions instead of just 50ml such as 120ml, 150ml. I could also compare this reaction with another one such as sodium thiosulphate; using sodium thiosulphate and hydrochloric acid. Change the concentration of the sodium thiosulphate solution and time how long it takes for an image of a cross drawn under the flask to disappear due to sulphur being precipitated. Another test is using marble chips and acid, measure how long it takes to collect a certain volume of carbon dioxide. A burette could have been used to measure the volume in place of the measuring cylinder. Overall though I feel this experiment went fairly well and am pleased with my results. ...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

    Rate of Reaction Chemistry Coursework

    4 star(s)

    doesn't have to stand and hold it up .Reaction Flask- We use this to perform the reaction in .Delivery Tube- We use this to allow the hydrogen from the reaction travel from the reaction flask to the burette .Measuring cylinder- We use this to measure the amount of hydrochloric acid

  2. Determine the rate equation for the reaction of hydrochloric acid with magnesium metal, and ...

    concentration graph equals minus the rate of reaction. This is further corrected for the initial gas lost below. The total gas produced in this reaction can be worked out theoretically. The magnesium is in excess so the moles of HCl consumed controls the moles of gas produced. 2HCl(aq)

  1. Rates of reactivity.

    * Both substances within the reaction were liquids so to control the surface area it will be very difficult. * No catalysts would be used. * I will use the same standard of time judged when the 'X' has disappeared.

  2. Find out how different concentrations of HCl affect the rate of the reaction with ...

    I also did the calculations to find out the mass of magnesium used and the volume of HCl used. CALCULATIONS. The equation for the reaction is: Mg(s) + 2HCl(aq) ----------> MgCl2(aq) + H2(g) The ionic equation for the reaction is: Mg (s)

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