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

Factors affecting the rate of reaction between Hydrochloric Acid and Magnesium.

Extracts from this document...


Factors Affecting the Rate of Reaction between Hydrochloric Acid and Magnesium I will be looking at how the concentration of hydrochloric acid affects the rate of reaction between hydrochloric acid and magnesium ribbon. I will need to time how fast this gas is produced to see how the rate of the reaction changes. The independent variable, the one that will change, therefore has to be the concentration of hydrochloric acid. The controlled variables are the ones which need to the kept the same to prevent unreliable results coming forth during the experiment. Collision Theory A chemical reaction can only occur between particles when they collide. Particles may be atoms, ions or molecules. There is a minimum amount of energy which colliding particles need in order to react with each other. If the colliding particles have less than this minimum energy, they will just bounce off each other and no reaction will occur. This minimum energy is called the activation energy. The faster the particles are going, the more energy they have. Fast moving particles are more likely to react when they collide. You can make particles move more quickly by heating them up, raising the temperature. ...read more.


I think this because the collision theory suggests that the more moving particles there are, the more collisions there will be and there will be a quicker reaction. I think every reaction will be quicker then the previous one and that the difference between the 0.4M experiment and 1.0M experiment will be quite substantial. Results; tables Here are the results from my experiment; they show the concentration of the hydrochloric acid, volume of hydrogen produce, and the two experiment times taken and an average worked out from the two times. 0.4 Molar Concentration H2 Volume (cm3) Experiment 1 Time (s) Experiment 2 Time (s) Average Time (s) 10 46 38 42 20 70 69 69.5 30 103 107 105 40 137 147 142 50 174 191 182.5 60 216 236 226 70 257 287 272 80 312 338 325 90 359 404 381.5 100 418 478 448 H2 Volume (cm3) Experiment 1 Time (s) Experiment 2 Time (s) Average Time (s) 10 17 17 17 20 29 30 29.5 30 43 45 44 40 59 58 58.5 50 74 74 74 60 91 91 91 70 108 109 108.5 80 127 130 128.5 90 148 150 149 100 172 177 174.5 0.6 Molar Concentration 0.8 Molar Concentration H2 Volume (cm3) ...read more.


The concentration and volume of the hydrochloric acid could have also been unreliable, although the use of burettes helped maintain a decent level of accuracy. The ideal method of measuring the volume and concentration of hydrochloric acid is to use industrial machines which are built to measure out chemicals very accurately. The surface area of the magnesium strip was one of the controlled variables which could have lead to anomalous results. This is because the surface area of the magnesium was not accurately measured; it was only assumed that if we use a 10 cm strip of magnesium there would be no fluctuation in thickness or width of the strip. This could have been improved if magnesium was accurately measured and cut with a cutting instrument, rather than by hand. Due to the lack of resources presented to us by school, students had to work together to get results which could be used, I have used the same results as a fellow student. My experiment could have been improved if I had completed it myself to my own personal level of detail and accuracy rather than it being done by a group of students where there are more openings for human error. Saqib Khan 11P 18.10.2003 ...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. Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric ...

    The quicker the rate of reaction, the less time the reaction will take to be completed. Therefore:- Rate of reaction 1 concentration of acid time taken to react So... Rate of reaction concentration time taken to react Plan I am intending to react a chosen length of magnesium ribbon with different concentrations of hydrochloric acid.

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

    The first is to find out what the initial rate of reaction would be for concentrations 1.25M hydrochloric acid and 1.75M hydrochloric acid as it would be interesting to see how the rate increases compared to 1M hydrochloric acid. Another experiment that I could do is change the type of acid that I use.

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

    1cm3 of HCL + 3cm3 water = 0.5M I will begin my investigation of volumes by using the above example and recording results in the table below. 4cm3 Concentration of HCL 2 M 1.5 M 1 M 0.5 M Time taken to react 44 seconds 1 minute, 35 seconds 3

  2. An Investigation into the factors affecting the rate of reaction between magnesium and hydrochloric ...

    As the temperature is increased the particles move faster since they have more energy. This means that they are colliding more often and more of the collisions have enough velocity to cause a reaction. Since there are more collisions the chemical reaction takes place faster.

  1. Investigation of some of the factors affecting rates of reaction.

    No catalyst will be provided for this reaction, so it cannot be used as a variable. Hence, the two variables which will be used are temperature and concentration. These variables are good ones in that they are easy to control and also easy to measure. A. HEAT (from Bunsen Burner)

  2. Investigation Into the Factors Affecting Rate of Reaction

    I will need to clean the conical flasks , beakers and thermometers because the bi-products of this experiment have been known to leave some sort of residue on the glass, therefore obscuring my vision and my results. Another good idea would be to label each flask as not to get them mixed up when doing my experiments.

  1. Investigating Factors Affecting the Rate of a Chemical Reaction

    increases.'* Therefore, increasing the temperature increases the energy between the particles and makes them move around a lot more and collide more often with each particle colliding and causing the reaction * 'www.chem4kids.com' Preliminary Results Using a set 5cm3 of 2 moles/dm3 of Hydrochloric acid (HCL)

  2. Investigate one of the factors affecting the rate of reaction between a metal and ...

    Safety: As I will be using glass conical flasks and burettes, I will be very careful when handling them in case I harm myself or others by dropping them. The hydrochloric acid is also corrosive, which means that it is able to eat away at materials that it is within contact with.

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