• 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...

Introduction

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.

Middle

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.

Conclusion

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. Factors Affecting Enzyme Activity

    It is possible that there were slightly different amounts of catalase in different samples of liver so this problem would be eliminated. In this project I intended to investigate the factors affecting enzyme activity. I then established that the main factors were temperature, pH and concentration of enzyme/substrate.

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

    To make sure that all my results are as accurate as possible I will do each experiment three times and then take an average to prevent any anomalous results affecting the end conclusion in a big way. Safety The safety of this experiment is very important.

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

    minutes, 7 seconds 13 minutes, 36 seconds These results show that with 4cm3 of liquid being used, the lower concentrations take far too long to react. If I use a larger volume of hydrochloric acid I can achieve concentrations in between more easily, such as 1.75 M I will now

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

    Note: They have been attached all overlaid their appropriate graph but should be viewed one at a time overlaid the appropriate graph. A tangent was drawn at the beginning of each curve and its gradient calculated, the gradients are shown in the table below.

  2. Investigation Into the Factors Affecting Rate of Reaction

    This could cause everything to go wrong as if I get the conical flasks muddled up then I would have to start from scratch due to atmospheric pressure differences. To ensure accuracy I will repeat my experiment twice, unless my results don't match, in which case I will attempt the experiment a third time.

  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. Investigating Factors Affecting the Rate of a Chemical Reaction

    and 50cm3 of 0.03moles/dm3 of Sodium Thiosulphate (THIO), I added these 2 reactants at different temperatures I found these preliminary results. Temperature (0C) (actual temperature in brackets) Time taken for reaction (s) Rate (1/time) (s-1) 20 (23) - room temperature 231 0.004 30 (32)

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