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

To find out what factors affect the rate of reaction between magnesium and hydrochloric acid, then investigate one of them in an experiment.

Extracts from this document...


INVESTIGATION IN THE FACTORS THAT AFFECT THE RATE OF A REACTION Aim=To find out what factors affect the rate of reaction between magnesium and hydrochloric acid, then investigate one of them in an experiment. Background Knowledge=A rate of reaction is how fast a reaction is between more than two reactants. They react with their particles, when they collide together they often do so with such a speed and force that they reach an 'activation energy', the energy needed for the materials to react. We know from past work and experiments, and also from official theories, that there are four main factors that affect the rate of reaction; these are categorised in the Collision Theory. ( this work was taken from CGP chemistry GCSE revision guide and Chemistry Counts textbook)) 1) Size of particles=When two materials are reacting together they can only do so with the area on the surface of the particle, obviously called 'surface area'. The larger that surface area is, the larger the area that they particles can react with, increasing their rate of reaction. This is explained in the diagram below 2) Catalysts= A catalyst is a substance which speeds up a reaction without being used up itself, eg, an enzyme is a biological catalyst. It does this by providing a surface that the particles stick to, so increasing the possibility that they will collide. ...read more.


Risk Assessment= Because of the acid being used safety precautions will need to be taken. Overalls and goggles will be warn, and extra care will be taken over spillages. Goggles will also be worn in case of any possible gases escaping and causing harm. Accuracy= I will try to be as accurate as possible when collecting my results, so I can be sure that my results are precise enough for me to form a strong conclusion. I will measure my liquids with the burette because it is more accurate and always rinse and dry out the conical flask between experiments, as any left over could influence the results. Variables= In my experiment I am only going to vary one thing; the concentration of the acid. I am going to do this by diluting the acid with water. I could not change more than one variable because then I would not be able to form a conclusion, as I would be unsure as to which factor made the difference. Fair test= To keep it a fair test, so to keep the results reliable I will vary and keep the same a number of things. The only thing I will vary is the concentration of the acid. I will keep the same burette, gas syringe, stop clock, ruler, type of HCL and type of Mg. ...read more.


The evidence I obtained is good enough to be used to simply prove/disprove my prediction. However, my individual results (i.e the specific ones for 1.0M/1.2M etc) would not be strong enough to prove/disprove anything as I do not think they are reliable enough. Repetition= if I was to repeat this experiment I don't think I would change anything about the procedure. For what I was trying to find out it was very appropriate and covered everything I needed to know. To improve my reliability I would measure the temperature all the way through and see how it affects my results. Future work=if I was to do any future work it would be to investigate another factor that affects the rate of a reaction. If I was to do temperature I would use the same concentration of acid all the way through and the same length of Mg ribbon but I would heat the HCl first and then time how long it took for the magnesium to dissolve. I would expect the results to be that there would be a higher rate of reaction (eg a faster time that the magnesium dissolved) the higher the temperature. This is because the heat energy gets transferred to kinetic energy in the particles, which makes them move about faster- so they are more likely to collide and reach their activation energy than at a lower temperature, when they are moving more slowly. 1 Jenny Wass, 11S ...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

    How dose temperature affect the rate of reaction between magnesium and hydrochloric acid.

    3 star(s)

    A stopwatch will be started when the reactants are placed together and stooped that they have fully reacted. If a gas produced then it will be easy to see when the reaction ends. It was not very hard to choose the method to do our practical with.

  2. Marked by a teacher

    For my experiment I am finding out the effects on the reaction rate when ...

    3 star(s)

    > Delivery tube- to get the hydrogen from the conical flask into the burette filled with water to measure the amount of hydrogen gas produced. > Stand with a burette clamp- A burette has a small base and is very tall so a stand and a burette clamp is needed

  1. Marked by a teacher

    The aim of this investigation is to investigate the rate of reaction of magnesium ...

    If I double the concentration of the acid from 1M hydrochloric acid to 2M hydrochloric acid then I will expect to see the rate of the reaction double. This is because there are twice as many acid particles in 2M hydrochloric acid than in 1M hydrochloric acid, so there will

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

    I carried out a preliminary test to measure how large the temperature increase would be. I found that when carrying out the reaction at room temperature, there was no measurable change in temperature from 23�C using the method described below.

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

    had just enough for 1 mole of magnesium to react with two of HCl. To get a fair reaction we had to keep the amount of magnesium the same and the temperature. We used 0.1g of magnesium. RESULTS Temperature From this graph you can see that if we do increase

  2. To investigate the factors which affect the rate of reaction between marble chips and ...

    45 Powdered Marble chips 60-20 30 = = 10 cm3 5-2 3 Medium Marble chips 73-15 58 = = 0.77 cm3 95-20 75 Small Marble chips 75-25 50 = = 1.66 cm3 60-20 30 Powdered Marble chips 64-30 34 = = 11.3 cm3 5-2 3 From these gradients it is

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

    Before starting the investigation, I decided to do some research about magnesium and hydrochloric acid. Magnesium is a light, shiny grey metallic element, symbol Mg, atomic number 12, found in group two in the periodic table. It is quite reactive giving vigorous reactions towards acids.

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

    take a while before it dissolves, and magnesium and hydrochloric particles react. The other 5 and the ways in which I am going to keep them constant are: * Concentration of hydrochloric acid: I will make sure that I use a constant molar of acid and to make sure that

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