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

An Investigation into the factors that affect the rate of the reaction between magnesium ribbon and dilute hydrochloric acid.

Extracts from this document...

Introduction

An Investigation into the factors that affect the rate of the reaction between magnesium ribbon and dilute hydrochloric acid Plan I predict that the higher the concentration of the hydrochloric acid, the higher the rate of the reaction. If the concentration of the hydrochloric acid doubles, the number of particles in the hydrochloric acid would double also. Therefore, the number of collisions between the particles will double so the rate would double also. This means that the rate of the reaction is directly proportional to the concentration of the hydrochloric acid. I worked this out by using the collision theory, where if you change the concentration, the rate changes in the same proportion. So the higher the concentration of the HCL the faster the reaction would take place, so the faster the magnesium ribbon would disappear. We can test if this prediction is correct for this reaction by measuring the rate of the reaction for a series of different concentrations. However we have to make sure we have a fair test by keeping all the variables the same except for the one we're studying. Final Method Before you start the experiment, the safety precautions need to be taken into concern first. A lab coat should be worn to protect yourself from the HCL you will be testing and any other chemicals in the lab, which could harm you. Safety glasses need to be worn at all times also. All other rules of the lab should be taken into concern before you start the experiment also. Firstly you need to set up the apparatus, which include: * Clamp & clamp stand * 100ml syringe * Two 100cm� cylinders * Side arm conical flask * Small beaker * Bung * Delivery Tube * Stop Clock Using a clamp and a clamp stand attach a 100ml syringe to it. ...read more.

Middle

0 0 5 10 10 17 15 23 20 26 25 28 30 31 35 33 40 35 45 37 50 38 Preliminary Experiment 4 Preliminary Experiment 5 2cm� HCL 1cm� HCL 3cm� Distilled Water 4cm� Distilled Water Time (secs) Amnt Hydrogen produced (cm�) 0 0 5 4 10 8 15 12 20 14 25 17 30 19 35 20 40 21 45 22 50 22 Time (secs) Amnt Hydrogen produced (cm�) 0 0 5 1 10 1 15 1 20 1 25 1 30 1 35 1 40 1 45 1 50 1 Fair Test To achieve a fair test in the experiment we need to list the factors, which could have an effect on the rate of the reaction in this particular experiment. These are the factors: * Temperature - kept the same at room temperature * Concentration of HCL- varied * Volume of HCL - varied * Size of Mg ribbon - kept the same at 10cm * Volume of distilled water - varied * Presence of catalyst - none Obtaining Evidence I repeated each experiment 3 times then I took the average. This was to make my experiment more accurate so it would be easier to test my prediction. Here are the results of my experiments: Expt 1: 50cm� HCL Expt 2: 40cm� HCL 0cm� Distilled Water 10cm� Distilled Water Time (secs) Hydrogen produced (cm�) 1st 2nd 3rd 2 25 9 23 4 54 27 54 6 65 48 78 8 74 67 88 10 79 77 91 12 79 84 92 14 79 86 92 16 79 86 92 18 79 86 92 20 79 86 92 22 79 86 92 24 79 86 92 26 79 86 92 28 79 86 92 30 79 86 92 Time (secs) ...read more.

Conclusion

The closer together they are, the more often the particles collide. The more often they collide, the higher the chance of a reaction between the magnesium ribbon and the hydrochloric acid. If you double the concentration of the hydrochloric acid , the number of particles in the hydrochloric acid would double also. Therefore, the number of collisions between the particles will double so the rate would double also. This means that the rate of the reaction is directly proportional to the concentration of the hydrochloric acid. I worked this out by using the collision theory, where if you change the concentration, the rate changes in the same proportion. The graph gives us a good device to prove that if you double the concentration the rate doubles also. Sources of error and limitations * I assumed that the room temperature was constant throughout the experiments. * The stop clock was unreliable and sometimes inaccurate because the second - hand was loose and would move if it were tapped. * The measuring cylinders used to measure the distilled water and HCL solution was only accurate to �1ml, so they're slightly inaccurate. * I washed and dried all our equipment but during the experiment dirt could've entered the side arm conical flask or water droplets could've been left in the flask. * When the reaction takes place bubbles of hydrogen are given off, which might stay around the magnesium, which therefore reduces the surface area of the magnesium and so the acid cannot react properly so this affects the results. * I could have stirred the solution more with a spoon because if this is not done properly it can lead to inaccurate 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

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

    4 star(s)

    placed above so that nothing can insert the conical flask during the experiment only the gas is allowed to get out. This strategy is used to see how long a solution takes to turn cloudy. It is used to see how long the reaction takes to dissolve making the cross on the piece of paper disappear.

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

    44 25 57 59 58 58 30 69 67 69 68 35 79 82 80 80 40 90 89 90 90 45 98 98 98 98 50 100 100 100 100 55 100 100 100 100 Concentration = 1.5 Molar Time (s)

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

    This is because at this point in the experiment there are more particles have not reacted in any way, and so there is more chance of an easy efficient reaction. In the middle of the experiment or at the second stage, the reaction has already been taking place and the

  2. The Iodine Clock Investigation

    Apparatus * H2O2 - 2 Vol. * KI -0.1M * H2SO4 - 1.0M * Na2S2O3 -0.005M * 2% starch solution * 50ml burettes (x5) * conical flasks * volumetric flasks * stands and clamps * funnels * stopclock * water bath (thermostatic)

  1. Rates of reactions between HCL and magnesium ribbon.

    The formula equation for this experiment is: Mg + 2HCl (r) MgCl2 + H2 Magnesium + Hydrochloric acid (r) Magnesium Chloride + Hydrogen The rate of reaction between the product and the reactant will increase or decrease depending on certain factors.

  2. Rate of reaction of hydrochloric acid and mangesium ribbon.

    with the magnesium with more energy, which will give more successful collisions per second. � Surface area of the magnesium If the magnesium had a bigger surface area each time the experiment was done, then the acid particles will have a bigger area to collide with, so more collisions will

  1. Free essay

    Magnesium Ribbon

    to occur and when these collisions occur, there is more chance that the collision will lead to a reaction. The particles will collide more often and thus the rate at which the product is being formed will also increase. This is because the amount of energy is more likely to

  2. Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

    Therefore, the magnesium atoms have more hydrochloric acid particles to collide with and the rate of reaction increases. This is again related to the collision theory. Also, in affect you are increasing the surface area of all the hydrochloric acid particles, and therefore there are more collisions.

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