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

Factors Affecting the Reaction Rate Between Magnesium and HCL.

Extracts from this document...

Introduction

Factors Affecting the Reaction Rate Between Magnesium and HCL Planning * Hypothesis I predict that as the temperature increases, the speed of the reaction will increase therefore the gas will be produced faster. I believe this because most chemical reactions happen faster when the temperature is higher. At higher temperatures molecules mover around faster, which makes it easier for them to react together. Usually, a rise of 10OC will double the rate of reaction. Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. 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. * Pilot Experiment To decide on the best volume and concentration of hydrochloric acid and best mass of magnesium a number of calculations were done and a pilot experiment conducted. The equation for the reaction is: Magnesium(s) + Hydrochloric Acid(l) Magnesium Chloride(l) + Hydrogen(g) Mg(s) + 2HCL(l) MgCl2(l) + H2(g) We were advised to use 0.1g of magnesium ribbon (found to be 10.9 cm long). The Relative Molecular Mass (RMM) of magnesium is 24, therefore the moles of magnesium to be used was: Moles= 0.1 24 Moles= 0.00416 In the reaction above, 1 mole of magnesium reacts with 2 moles of hydrochloric acid. ...read more.

Middle

A 100cm3 gas syringe should be appropriately accurate for measuring the gas produced since it is accurate to 1cm3 of gas. I will use a three figure balance to measure the mass of magnesium to be used since it is vital that as close to 0.1g of magnesium is used as possible. * Variables I have chosen to repeat the experiment 3 times because it therefore allows me to calculate an average rate of reaction. This will ensure that there are no abnormal results and it will increase accuracy. I have decided to start readings at 20OC and increase by 10OC each 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. The faster the particles move, the greater the number of collisions, and therefore the rate of the reaction increases. A 10OC rise in temperature almost doubles the rate of most reactions. Chemical reactions take place by chance. Particles need to collide with enough velocity so that they react. 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. ...read more.

Conclusion

Although the initial rate of reaction (which is what I am concerned with in this investigation) seemed to fit a trend, the rate of reaction curves of some temperatures on the graphs crossed. This could have been because some of the magnesium had corroded forming a magnesium oxide layer which would have affected the rate of reaction. Other factor which could have given me unreliable results could have been that the gas syringes were wet causing them to jam and so not giving correct results or that the bung was not placed on the top of the side arm tube fast enough which allowed gas to escape. I conducted all three experiments for each temperature at the same time to save time. An error in my graphs (plotting, drawing curves or calculating gradients) could have also affected the calculated rates of reaction. To improve the experiment I would find a way of attaching and releasing the magnesium inside the side arm tube above the acid (with a bung at the top of the side arm tube) so that the magnesium could be dropped into the acid without any gas being lost. Additional work, which could be carried out, is to repeat the experiment using, a wider range of temperatures. The investigation could also be extended to investigate other factors affecting the rate of reaction such as catalysts, concentration of the acid or particle size of the magnesium. ...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. Investigating the Rate of Reaction Between Hydrochloric Acid (Hcl) and Magnesium (Mg).

    So therefore from that graph, knowing the rate of reaction is quickest on the steepest gradient, you can find out that when the temperature was 60oC the reaction was fastest This happens because of both the collision/kinetic theory and because of activation energy.

  2. Rates of reaction between Magnesium and HCl.

    I would dilute it by water in order to obtain the concentration required. Initially I used 2M hydrochloric acid, but the reaction seemed extremely fast, and would not enable me to record accurate results, as the times were extremely close, and from using my own judgement, using a 2M acid seemed not appropriate.

  1. Investigate the factors affecting the rate of a reaction.

    I also will record these results also. Since these numbers will be small and quite complicated I am going to add a further column to my final table of results and record the answers in standard form. After doing this I will have a complete set of results ready for analyzing and comparing.

  2. Factors Affecting Enzyme Activity

    my results, fortunately the pH of my reactants were all seven so this could not have affected my results. However, the temperature of my experiments fluctuated by *****degrees. Given that this is only a small temperature difference and my results still appeared to fit the pattern I predicted I think

  1. Rates of reactions between HCL and magnesium ribbon.

    Then I will be ready with the stopwatch and then quickly drop in the ribbon into the acid, and start the stopwatch. This must all be done in a very short space of time. I must record the results in a table and then write it up neat later.

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

    Analysing Evidence First three graphs were drawn (one for each time the whole experiment was carried out). So that the graphs did not become over crowded the curves were drawn on separate pieces of see through OHP film and overlaid each graph.

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

    the molecules of oxygen and nitrogen in air are colliding but do not react as the temperature is not high enough. But if the temperature is raised, for example in a lightning bolt or in a car engine, then they can react.

  2. Investigation Into the Factors Affecting Rate of Reaction

    This supports my first prediction about the rate of reaction on the sodium thiosulphate. The second point shows that more time has taken for the marble chips to react completely. This tells me that less successful collisions happen per second.

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