• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9

Acid and Metal Reaction Investigation

Extracts from this document...


Planning The reaction of an acid with a metal is a good way of producing hydrogen in the laboratory. Usually a moderately reactive metal is used as this means the hydrogen doesn't come off to quickly or slowly. Zinc is quite often chosen e.g. Zinc + Sulphuric acid --> Zinc Sulphate + Hydrogen The reactivity of metals with acid can cause corrosion problems where there are acidic gasses in the air. An example of an acidic gas is Sulphur dioxide. It pollutes the air in industrial areas causing acid rain. This acidity sometimes makes cars, bridges, statues etc corrode. All metals react the same when above hydrogen in the reactivity series, an example of an equation of this is: Metal + Acid --> Metal Salt + Hydrogen All substances are made up of particles, reactions only occur if reacting particles collide together, this is called the collision theory. Collisions are only successful if the collisions exceed the minimum activity energy. You can increase the rate this reaction occurs by increasing the number of collisions per second, or increase the average force of collisions. Some factors that will affect the rate of reaction are the temperature of the room and the solution. The higher the temperature the quicker the reaction. The concentration of the solution also affects the reaction rate as the greater the amount of acid then the greater the rate. ...read more.


75 74 74 14 16 95 96 96 96 Apparatus * Sulphuric Acid * Water * Beaker * Stirrer * Magnesium Ribbon * Burette Analysis My first graph shows the time it takes a 1cm piece of magnesium ribbon to dissolve in different concentrations. The time is done in seconds and the concentrations in ratios e.g. 14/16 The graph clearly shows that the more acid in the concentration the less time it takes to dissolve. Therefore the more dilute the acid is the longer the magnesium will take to dissolve. The results of the experiment fit in with my prediction that the higher the concentration of acid the less time the magnesium will take to dissolve. This is because the acid is less dilute which means that the pieces of magnesium will dissolve slower than a more concentrated solution. This occurs as there would be less meaningful collisions. I found no anomalous results in my experiment. This may be because the readings were taken in controlled circumstances so we were able to perform a fair test. I believe that I should draw another graph to find out the rate of reactions. I will do this by using the equation. Speed = Distance Time Speed will represent the rate of reaction ( this is what we want to find out ). ...read more.


I found no big anomalous results on my graphs, when doing the experiment I took averages which helped to filter out any anomalous results from my readings, but even I these my results seemed quite constant. I believe I made my experiment a very fair test. I measured the acid and the water out carefully to ensyre the concentration was correct. I also stirred constantly on every concentration to make sure we has similar results and keep a fair test. The results on my graphs reflect this by following a curve and line of best fit. Due to the small amount of solution we used the smaller concentrations there became less sulphuric acid particles which meant there was a less effective collisions. The only way this could have been prevented if there was a infinite amount of acid which would make the loss of concentration irrelevant. We could improve the experiment by using a micrometer screw gauge to measure the magnesium ribbon more accurately. This would ensure that we had the same surface area on each magnesium piece. We could also use a stirring mechanism to ensure constant stirring. This would solve any problems we had with not being able to keep it constant by stirring manually e.g. tiring after stirring for a period. To further this experiment we could maybe try doing different lengths of magnesium or change the surface area. This would enable us to see what happened if there was less or more surface area. ...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 Aqueous Chemistry 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 Aqueous Chemistry essays

  1. Investigate whether temperature affects the rate of reaction between Magnesium ribbon and Sulphuric acid.

    When they collided in the experiment the gas was given off therefore the faster the particles moved, the more particles collided, giving off more gas. The results table proves my prediction, where I said that more gas would be produced at a higher temperature.

  2. Reactivity of metals Investigation

    This means that calcium is the most reactive metal out of the four metals available. Also just by looking at the reaction you can tell that it is the most reactive.

  1. What affects the reaction rate between magnesium and sulphuric acid?

    Time (seconds) 50 0 50 19 40 10 50 27 30 20 50 34 20 30 50 57 10 40 50 126 I have also drawn out a scatter graph to show the results. This is a table to show the results averaged out between the two experiments.

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    x 7.17 cm3 1000 The volume of the average titre is divided by 1000 to change the units from cm3 to dm3. Moles = 0.00017925 mol dm-3 The ratio of Potassium Manganate (VII) (aq) to Iron (II) (aq) is 3:5 and therefore to work out the mols of Iron (II)

  1. Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress ...

    The concentration 0.06mg/l of copper sulphate, which was closest to the natural level, had the lowest standard deviation other than the 60mg/l of copper sulphate. This shows that in each batch almost the same number of seeds germinated, showing that this concentration was consistently right for seed germination.


    * The hydrogen peroxide should be measured out accurately. The oxides should also be weighed accurately using an accurate balance. * The oxides should all be in solid powdered form and not in any other form, as this will effect how the catalysts react with the hydrogen peroxide.

  1. Reactivity Series Investigation

    did not react with the cold hydrocholic acid.I would like to repeat my experiment with the cold acid 5 times to make the result more reliable and I would like to repeat my experiement with the warm acid 5 times to make it into a fair test and make sure that my results are more reliable.

  2. whether the strength of Hydrochloric acid will affect the speed of the rate of ...

    bunk into the top and start the stop watch, but this is impossible so we just have to do it as fast as we can whilst still being safe in what we are doing. Once we have done this we then record results every 5 seconds until the experiment runs

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