• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
Page
  1. 1
    1
  2. 2
    2
  3. 3
    3
  4. 4
    4
  5. 5
    5
  6. 6
    6
  7. 7
    7
  8. 8
    8
  9. 9
    9
  10. 10
    10

Reactivity Series Investigation

Extracts from this document...

Introduction

Experiment on Metals Aim-To find out which of these metals will be most reactive with hydrochloric acid,and plan an investigation to test it out.The Metals given:Calcium,Aluminium,Iron,Magnesium and Zinc. Prediction-I predict that the metal will be the most reactive with hydrocholoric acid is calcium because calcium is in Group 2 which is the alkaline earth metals in the periodic table and because calcium is at the extreme left side of the periodic table and as you go across a period,the element change from reactive metals on the left to non reactive metals on the right.On the extreme right of the periodic table is the noble gases.Also calcium is Group 2 which is the alkaline earth metals and they are part of the reactive metals which is Group 1 and 2.Also out of all of the metals given calcium reacts more faster with air and creates a sparkling sight and can damage your eyes creating calcium oxide in word equation it is Calcium+Oxygen equals calcium oxide.In chemical equation it is 4Ca +O2 equals 2 Ca2o.Calcium also reacts more than zinc,aluminum,iron and magnesium with water and much more violent and quicker creating vapour and moves much faster than the other metal and creates a vigrous sizzling sound and fizzing in water and dissloves much faster than the other metals. The alkaline metals get more reactive as you go down the group and calcium is further down than magnesium so therefore it must be more reactive than magnesium. Calcium is in group 2 in the periodic table which is more reactive than iron and zinc in the transistion metals section of the periodic table which is not very reactive because transisiton metals are the metals they use to build structures or making things since they have high melting points and high densities.Calcium is in group 2 and is the more reactive out of all the metals is because group 2 metals in the periodic table have low melting points than the transition metals which iron and zinc ...read more.

Middle

to non reactive metals on the right.On the extreme right of the periodic table is the noble gases.Also calcium is Group 2 which is the alkaline earth metals and they are part of the reactive metals which is Group 1 and 2.Also out of all of the metals given calcium reacts more faster with air and creates a sparkling sight and can damage your eyes creating calcium oxide in word equation it is Calcium+Oxygen equals calcium oxide.In chemical equation it is 4Ca +O2 equals 2 Ca2o.Calcium also reacts more than zinc,aluminum,iron and magnesium with water and much more violent and quicker creating vapour and moves much faster than the other metal and creates a vigrous sizzling sound and fizzing in water and dissloves much faster than the other metals.The alkaline metals get more reactive as you go down the group and calcium is further down than magnesium so therefore it must be more reactive than magnesium. Calcium is in group 2 in the periodic table which is more reactive than iron and zinc in the transistion metals section of the periodic table which is not very reactive because transisiton metals are the metals they use to build structures or making things since they have high melting points and high densities.Calcium is in group 2 and is the more reactive out of all the metals is because group 2 metals in the periodic table have low melting points than the transition metals which iron and zinc belong to and The 'poor metals' which aluminium belong to and they also have low low densities than the other metals and this agrees with my predictionand that calicum is in a higher position in the reactivity series so therefore it is more reactive than magnesium,aluminium,zinc and iron when it is reacted with air or oxygen,water or steam and therefore is the most reactive in reaction with hydrocholic acid.The product or the result of the reaction of hydrocholic acid and calcium is calcium chloride+hydrogen gas which is the gas ...read more.

Conclusion

40 or 50 secs so we can see the reaction of iron and aluminium which reacts very slowly.There should be results backing up the conclusion by doing further work and get a longer gas syringe where I can read off the amount of hydrogen gas each metal is giving out because there are results for the calcium experiment and the magnesium experiment have gone over the limit for the gas syringe so we need a longer one to make the results reliable.There should be more results to back up the conclusion as I myself are not sure if the conclusion is valid and right because of so many things went wrong.We should also have repeated the experiment at least five times to make sure it is right and then we can make an postive conclusion to this experiment.Also aluminium and iron do not react well with hydrocholic acid but Aluminium metal dissolves readily in dilute sulphuric acid to form solutions containing the aquated Al(III) ion together with hydrogen gas, H2. The corresponding reactions with dilute hydrochloric acid also give the aquated Al(III) ion. Concentrated nitric acid passivates aluminium metal. 2Al(s) + 3H2SO4(aq) 2Al3+(aq) + 2SO42-(aq) + 3H2(g) 2Al(s) + 6HCl(aq) 2Al3+(aq) + 6Cl-(aq) + 3H2(g) Iron also dissolves well with sulphuric acid as iron metal dissolves readily in dilute sulphuric acid in the absence of oxygen to form solutions containing the aquated Fe(II) ion together with hydrogen gas, H2. In practice, the Fe(II) is present as the complex ion [Fe(OH2)6]2+. Fe(s) + H2SO4(aq) Fe2+(aq) + SO42-(aq) + H2(g) If oxygen is present, some of the Fe(II) oxidizes to Fe(III). The strongly oxidizing concentrated nitric acid, HNO3, reacts on th surface of iron and passivates the surface.So I think that a different kind of acid should be used like sulphuric acid to see a reaction properly as aluminium and iron do not react well with hydrocholic acid.My plan could be improved by adding sulphuric acid to be reacting with the metals instead of hydrocholic acid. ...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 the factors, which affects how quickly Calcium carbonate reacts with hydrochloric acid.

    The successful collisions are the one where the particles hit head on and the particles contain high energy and this by increasing the temperature. Fig2 raising the temperature speeds up a reaction In my prediction had stated that as you increase the temperature, the reactants will react faster with each other .I had explained this using the kinetic of matter.

  2. Reactivity of metals Investigation

    Aluminium 7. Zinc 8. Iron 9. Tin 10. Lead 11. Copper 12. Silver 13. Platinum 14. Gold Prediction I predict that calcium will give a more vigorous reaction and give off more heat. This is because calcium is higher up in the reactivity series than any other metal used in this experiment.

  1. Why do penguins huddle to keep warm?

    65 63 62 61 60 58 57 55 54 53 53 4 70 67 65 62 61 59 58 57 56 54 53 52 51 5 70 67 64 61 59 57 54 53 51 48 46 44 43 On the preceding page is the control experiment which done to

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

    Add distilled water (l) to the volumetric flask until it is about 1cm below the graduation mark. g. Slowly add the distilled water (l) using a clean dropping pipette until the bottom of the meniscus is touching the graduation mark. h. Stopper the flask and invert it several times.

  1. Electronic spectroscopy - Homoleptic chromium(III) complexes and the spectrochemical series.

    The complex [Cr(NH3)6]Cl3 was prepared as follows. A pre-calibrated vacuum trap tube (B29) was half-immersed in an acetone/dry ice mixture (kept cold throughout by the regular addition of CO2) in a Dewar flask and connected to an ammonia cylinder. Liquid ammonia was collected to the 40cm3 mark.

  2. Determining the purity of Iron Wool.

    Using this reading along with a series of calculation and balanced reaction equations the percentage purity of the Iron wool was calculated to be 74.20%. We can assume this result to be the correct percentage purity of Iron wool however from other experiments along the same lines the percentage purity calculated was lower than anticipated.

  1. My aim is to put zinc, iron, magnesium, nickel and calcium into an order ...

    Nickel will hardly react. Method * The things that will change in the experiment are the temperature * I will carry out the experiment by putting the metal powder in a test tube and then mixing with it hydrochloric acid and I will measure the temperature every 30 seconds for five minutes.

  2. To organise 5 given metals into a reactivity series using 0.2 M Copper (II) ...

    If we add too much metal than some of that metal will not react with the copper (II) sulphate. So we must add copper sulphate solution in excess, so all the metal reacts. To make sure that the copper sulphate is in excess I will work out how much of each metal will react with 20cm3 of Copper Sulphate Solution.

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