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

Investigating varying concentrations, affecting the Rate of Reaction between hydrochloric acid (HCL) and magnesium (Mg)

Extracts from this document...

Introduction

GCSE Chemistry Coursework Investigating varying concentrations, affecting the Rate of Reaction between hydrochloric acid (HCL) and magnesium (Mg) Candidate name: Alexander Willink Aim: The aim of this experiment is to find out the effect of concentration of acid, in the reaction between dilute hydrochloric acid and magnesium ribbon. Prediction: I predict that with an increase in concentration the rate of reaction will there for also increase. This will (I predict) be proven by the amount of hydrogen gas produced. If we increase the concentration, we are in essence, increasing the total number of collisions. This, in turn, will increase the number of effective collisions, and the rate will increase. Introduction: magnesium + hydrochloric acid magnesium chloride + hydrogen Mg (s) + 2Hcl (aq) MgCl2 (aq) + H2 (aq) For a successful collision reaction to take place the reacting particles must collide with enough energy, this energy will need to be sufficient to break the magnesium bonds. Room temperature should be adequate. The rate of reaction can be measured by how many successful collisions occur in units of time, (the amount of hydrogen gas produced). When the concentration increases, so will the reaction. This is because there should be more particles to react with the magnesium. Whilst magnesium and hydrochloric acid particles are making successful collisions their particles are forming magnesium chloride and hydrogen. ...read more.

Middle

when the Concentration of HCL increases. The theory states that if, the more concentrated the Reactants, the greater the number of collisions between particles increases. This also explains why the greatest rate of reaction is usually as soon as the reactants have been mixed, i.e. they are both at their highest concentrations. As the reaction continues, the Concentration of the reacting substance decreases and so does the rate of reaction. We must consider what happens when a reaction takes place. First of all the particles of the Reacting substances must collide with each other, and secondly a fixed amount of energy Called activation energy* (Ea) must be reached for the double bonds to be broken into single ones. If the Particles can produce the right amount of energy (i.e. if they collide fast enough and in the Right direction) a reaction will take place. The reaction is speeded up if the numbers of Collisions are increased. In this investigation we must consider the topic of variables. Clearly, the time taken for the magnesium to disappear when it is placed in different concentrations of HCL is related in some way. The higher the concentration of HCL you use, the less time it takes for the magnesium to disappear and so the rate reaction increases. The concentration of HCL you use is the independent variable because it will Vary, and the time taken for the rate of reaction to take place (i.e. ...read more.

Conclusion

I submitted all the results to a computer program called excel, where, by using a formula, I was easily able to subtract each starting value from each set of results. By doing this, it would create the illusion that all experiments started at 0cm�. 7. I should have been more accurate in cutting the magnesium; my graphs prove that the magnesium was cut inaccurately. I would expect all the results to end at the same level. This, however, is not the case. One other explanation of the inaccuracy (you must understand I am trying to shift the blame a little) is the constant minor change in room temperature, emphasized by the fact that the tests were not executed all in the same setting. 8. I could also have gained more results by simultaneously recording the temperature. I could then ensure that the reaction was taken whilst in similar temperature conditions....different temperatures. How is done. 9. Another anomaly that is clearly spotted in the graph is the different concluding results for each experiment. I expected all the results to level out at roughly the same level. However there is a clear difference between 10. The line of best fit drawn from the graph can see the accuracy of the results. If it is clear that a point is not following the line, then it can be accounted for as an anomaly. There may be many reasons for such an occurrence. 1 1 GCSE Chemistry Coursework Alexander willink Chemistry coursework 2003 Page 1 of 1 ...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)

    With a smaller size of magnesium the speed is increased. Magnesium which has a smaller size in particle reacts more quickly than solids which have a larger size in particle. The acid starts to react from the edge of the magnesium this means that it takes longer for the reaction to finish.

  2. Marked by a teacher

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

    3 star(s)

    > Large thermometer- to measure the temperature of the solution before and after the reaction to get an average temperature of the solution during the reaction. It is important as a small difference in temperature causes a big difference in reaction rate.

  1. Rates of reaction between Magnesium and HCl.

    Then record the results in a table. Repeat for each of the temperatures shown in the table below. Temperature (� C) Time for cross to disappear (seconds) 20 117 30 27 40 24 50 12 60 7 70 4 From this experiment, I am able to show that as the temperature increases, so does the rate of reaction.

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

    This heat energy will then be converted into kinetic energy and the atoms will collide more often. So if you increase the temperature you increase the amount of kinetic energy and therefore, increase the rate of reaction. The collision theory comes into play concerning the speed.

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

    This would only produce a first order dependence on concentration since only one hydrogen ion is involved. The pathway is therefore not confirmed by my results. Limitations If I had time I would have liked to use a gas syringe to collect the hydrogen from the boiling tube.

  2. Factors Affecting Enzyme Activity

    With very specialist equipment it would be possible to extract the enzyme and so I could make solutions of catalase. This would give me more accurate results as there would be no discrepancies whatsoever with regards to the amount of catalase.

  1. To investigate the effect of varying the masses of white sugar and yeast and ...

    of dough/ml 0 30 30 30 1 30 30 30 2 30 30 30 3 30 30 30 4 30 30 30 5 30 30 30 6 30 30 30 7 30 30 30 8 30 30 30 9 30 30 30 10 30 30 30 11 30 30 30

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

    time until 60OC is reached, since it will allow me to see the increase in rate of reaction and 5 results should be enough to identify any trends. * Rates of Reaction Increasing the temperature increases the speed of the particles.

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