• 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

Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid.

Extracts from this document...


Rates of Reaction: Investigation Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid. Chemical reactions between substances are caused by the collision of particles. More collisions mean a quicker rate of reaction. In the reaction between hydrochloric acid and magnesium ribbon, the chemical reaction takes place when the magnesium ribbon is dropped into the hydrochloric acid. The products are hydrogen gas and magnesium chloride. The equation for this reaction is as follows:- Magnesium + Hydrochloric acid Magnesium chloride + Hydrogen Mg (s) + 2HCL (aq) MgCl2 (aq) + H2 (g) Factors that affect the rate of reaction:- * Temperature * Mass of magnesium ribbon * Concentration of hydrochloric acid * Surface area of magnesium ribbon I have chosen to use the concentration of hydrochloric acid as my independent variable. These different concentrations can be varied easily and made up accurately for the experiment. Each experiment will be done four times so that an average reading can be calculated - ensuring an accurate and reliable conclusion. The measured variable will be the time taken for the same quantity of magnesium ribbon in each experiment to be used up in reaction. The constant variable will be the length of the magnesium ribbon used in each experiment. Rate of reaction = Gradient of the line of a graph plotted with time taken to cease reacting against concentration. ...read more.


Each 1cm quantity of magnesium will be cleaned with emery paper before use to eliminate contamination from other chemicals which may be on the surface. Each beaker of hydrochloric acid will be used only once. The 1cm lengths of magnesium will be measured and cut as accurately possible using a ruler with millimetre measurements and sharp scissors. The stop-clock used will be accurate to the nearest second. The variable I will change in each experiment is:- � The concentration of hydrochloric acid. The apparatus and chemicals used for my experiment will be as follows:- � 2 large beakers. � 5 conical flasks � a large measuring cylinder (that holds up to 25cm3 of liquid) � supply of 2M concentration hydrochloric acid � roll of magnesium ribbon � supply of distilled water � stop-clock � ruler Safety Throughout all experiments I will be cautious when handling chemicals and wear the following safety items at all times:- � lab coat � safety goggles Method One large beaker was taken and filled with 2M hydrochloric acid. Another large beaker was taken and filled with distilled water. A stop-clock was taken and set aside. Five conical flasks and a measuring cylinder were taken. The measuring cylinder was used in the following way to achieve different concentrations:- 25cm3 of HCL = 2 mol.dm-3 21cm3 of HCL + 4cm3 water = 1.75 mol.dm-3 19cm3 of HCL + 6cm3 water = 1.5 mol.dm-3 12.5cm3 of HCL + 12.5cm3 water = 1 mol.dm-3 6cm3 of HCL + 19cm3 water ...read more.


I also checked my calculations with a calculator to make sure I had not mad any errors. I did have one anomaly in my results, which was the rate of reaction (gradient calculation) for 1.75M. This rate of reaction was 0.01 higher than the 2M rate of reaction, going against my prediction and causing an abnormality in the curve on my graph. This may have been caused by the acid used to make up/water used to dilute the 1.75M of hydrochloric acid being at a higher temperature than the rest. If the liquid were at a higher temperature, the particles inside would have more energy and so be moving around faster. This would mean HCL and magnesium particles would collide more frequently, thereby increasing rate of reaction. I think that my results on graph 1 were suitable to draw an accurate best-fit line. The points are all joined by the line. I used 5 different concentrations which were in a suitably wide range. If I were to repeat the experiment I would use a slightly wider range of concentrations to expand my conclusion, such as 1.25M, 0.75M and 0.25M. If the resources were available, I would also extend the range to higher concentrations than the 2M I was restricted to in this investigation. Further investigation could also include using another factor as my independent variable. I could differ the surface area of magnesium in my experiments, and see how this affects rate of reaction; in what way and if there is a definite proportional relationship. ...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

    Investigation of the rate of reaction between Magnesium and Hydrochloric acid

    4 star(s)

    Had a good set of results Seventh test: Hydrochloric acid 0.6 molar (50 ml) and calcium carbonate powder (0.5 grams) Hydrochloric acid 0.6 molar (50 ml) and calcium carbonate powder (0.5 grams) Seconds (s) Gas produced (cm3) 0 0 30 34 60 38 90 44 120 46 150 46 180

  2. Marked by a teacher

    The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric ...

    4 star(s)

    7 6.33 0.07 120 8 7 8 7.67 0.06 150 10 11 10 10.33 0.07 180 13 14 13 13.33 0.07 Safety Safety/Risk Assessment: For this investigation I will take specific cautions when investigating how different concentrations effect rate of reaction, this will be done before we start with our experimentation in order to fulfil our investigation.

  1. Investigating the rate of reaction between Magnesium Ribbon and Hydrochloric Acid.

    I will then fill one of the 100cm3 beakers with hydrochloric acid and the other beaker will be filler with distilled water. I will also cut a 10 cm strip of magnesium ribbon, and weigh it with the balance. Having taken it all to the bench where I am working

  2. Finding the effect of concentration on the rate of reaction of magnesium ribbon with ...

    The inaccuracies could have also been caused by the magnesium strip varying slightly in length and volume of hydrochloric acid not being in exactly the same quantities or concentration. Also the gas syringe throughout the experiment could have been stuck and as the pressure increased the syringe could have jumped

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

    Method I intend to find the rate of reaction at different temperatures by measuring the amount of time it takes for a small amount of magnesium powder to react completely with an excess of HCl. The reaction ends when the powder disappears and no more bubbles are produced.

  2. Rate of reaction between magnesium ribbon and hydrochloric acid.

    The reaction between HCl and magnesium ribbon is exothermic. Which means heat is given out. During a chemical reaction, old bonds are broken and new bonds are formed. Energy is released when new bonds are formed, so bond formation is an exothermic process.

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

    Altogether I tested 5 different concentrations of hydrochloric acid. 0.0M, which was the lowest concentration of acid that I used, there was no reaction. 2.5M hydrochloric acid, which was the highest concentration that I used, produced the fasted rate of reaction.

  2. Investigating Factors Affecting the Rate of a Chemical Reaction

    exact same equipment and done it in the exact same environment to make absolutely sure that the experiment was fair at each temperature. I think that these were both very important factors because they could affect the results severely and leave me with an anomalous when I should only have correlating results.

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