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

An investigation into the rate of reaction between magnesium and hydrochloric acid.

Extracts from this document...

Introduction

An investigation into the rate of reaction between magnesium and hydrochloric acid. Aim The aim of this experiment is to see how a variable will alter the rate of reaction between magnesium and hydrochloric acid. Magnesium is comparitvely highly reactive. It burns in oxygen with a white light and reacts quickly and vigorously with hydrochloric acid. The magnesium bubbles and fizzes in the hydrochloric acid. The reaction is an exothermic reaction and lasts for only a short period of time. The gas given off from the reaction is hydrogen, and a small amount of magnesium chloride solution is left in the beaker. The word and symbol equation for the reaction: Magnesium + Hydrochloric acid Magnesium chloride + Hydrogen Mg + 2Hcl MgCl2 + H2 Solid Liquid Liquid Gas Preliminary Work I have carried out some preliminary work prior to this investigation, involving rates of reactions. From these I found out about the collision theory. More particles of the acid are available; therefore there was more chance that the H+ ions in the acid would collide. I tested the rates of reactions with hydrochloric acid and magnesium ribbon. In this experiment I was looking at how magnesium reacted with hydrochloric acid at different strengths (using water to dilute the acid). ...read more.

Middle

Problems I expected some problems to occur during the experiments, however there was really only one upset. This was the fact that when I tested the 0.2M it was very slow and took a long time. So long that I did not have time to finish the experiment. It took over 50 minutes and was inconclusive. Therefore I decided to test more concentrations of hydrochloric acid to make up for my loss. However I could not test 0.9M, as this would upset any trend in my concentrations, therefore I decided to test extra four concentrations: 0.3M, 0.5M, 0.7M and 0.9M. I now had a collection of eight concentrations. A problem with making these concentrations was that I had to use 50ml of solution to prepare them. Therefore I decided to just half the concentrations I made up to give me 25ml. Below is a table showing the dilutions of extra the concentrations: Concentration (M) Amount of Hcl (ml) Amount of H20 0.9 45 5 0.7 35 15 0.5 25 25 0.3 15 35 I tested these concentrations exactly as I did the others and recorded my results. I was pleased with this modification as it allowed me to test a wider range of results to give me a clearer picture and more accurate readings. Results First set of results Concentration Hcl (M) Time taken for Mg to disappear(s) ...read more.

Conclusion

If I had done the opposite end tested smaller molarities for example :0.1(M) the experiment would have taken a very long time, this is because there are not as many molecules available to react in the Hcl and it would have taken a lot longer for the magnesium atoms to find and collide with the Hcl molecules. Evaluation From this investigation I think that I have achieved my aim of finding the affect that surface area of the magnesium ribbon had on the rate of reaction between the hydrochloric acid and magnesium. I think that I obtained enough results to give me a detailed graph and conclusion. I was pleased with my results and were very accurate given the conditions of a classroom. I am pleased with how my graph formed, from it I can tell that the surface area is proportional to the rate of reaction, as was predicted. There are no major anomolos results which shows that my experiment was carried out with some accuracy. If I could repeat the experiment I would try to make it more accurate, If possible I would use more accurate and precise equipment. I would have used a ruler with smaller divisions to measure the size of the magnesium ribbon. I would also like to use some kind of machine or incubator to keep the experiment at a constant temperature. ...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)

    9 0.90 1.24 20 29 26 18 24.33 1.22 30 37 39 36 37.33 1.24 40 37 40 38 38.33 0.96 50 37 40 38 38.33 0.77 60 37 40 38 38.33 0.64 0.5 30 0 1 1 0.67 0.02 0.07 60 3 4 4 3.67 0.06 90 6 6

  2. Marked by a teacher

    Investigation of the rate of reaction between Magnesium and Hydrochloric acid

    4 star(s)

    Table 3: - Showing the volume of gas produced by a reaction between calcium carbonate and a 0.6M concentration of acid. Hydrochloric acid (50 ml) (0.8 molar) + Calcium Carbonate (0.5g) Volume of gas produced in cm3 Time (sec) 1st test 2nd test 3rd test 4th test Average Range 0

  1. Marked by a teacher

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

    3 star(s)

    It is calculated by: Average rate = Change in volume of hydrogen Time taken for that volume of hydrogen gas to be produced The rate of reaction tells us what rate the graph is going, for each concentration at a particular time.

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

    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

  1. Rates of reaction between Magnesium and HCl.

    Average rate of reaction (cm�/second) 1.0 0.25 0.9 0.21 0.8 0.15 0.7 0.12 0.6 0.09 0.5 0.06 0.4 0.05 0.3 0.03 0.2 0.02 0.1 0.01 From the graph above it is clear that as the concentration of the hydrochloric acid increases, so does the average rate of reaction.

  2. Finding the effect of concentration on the rate of reaction of magnesium ribbon with ...

    of 2 moles would be double the time of a 1-mole solution. When also using the same quantities of reactants, the product that is produced will be the same. Results table that was used to create a graph that resembled my theory.

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

    it gives out heat) which means the temperature of the solution will increase. This is because when bonds are broken (in our case hydrogen and chlorine) they use up energy, and when new ones are formed they they give out energy.

  2. How does changing the concentration of hydrochloric acid affect its rate of reaction with ...

    15 cm strip of magnesium, which is in excess and enough for all the acid to react. Overall; this preliminary study has helped me to get familiar with the method and the apparatus I will have to use in the main experiment.

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