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

Investigation to find out what affect the position of a metal in the reactivity series has on its ability to be displaced.

Extracts from this document...


Johanna Mans 12.2 Enthalpy changes on displacement and the reactivity series Aim To find out what affect the position of a metal in the reactivity series has on its ability to be displaced. Background Information The reactivity of metals is shown in the reactivity series below. Potassium Most reactive Sodium Calcium Magnesium Aluminium Zinc Iron Lead Copper Silver Gold Platinum Least reactive As zinc is higher in the reactivity series than both lead and copper, it will be able to displace them from their compounds. Hypothesis The closer the metal is to zinc, the harder it will be for zinc to displace, eg, iron would be harder for it to displace than silver. This means that less energy will be produced. Therefore, I predict that lead will be harder to displace, and will therefore have the smaller enthalpy change value. Apparatus Justification Apparatus Justification Polystyrene Cup This acted as the calorimeter, and this is an insulator to ensure that it is not effected by the heat changes in the ...read more.


It is an irritant so if spilt on labcoat or skin, the area should be washed immediately. Diagram Method 1. The calorimeter was set up as shown in the diagram above. This was done by placing a polystyrene cup inside a glass beaker. 25cm� of 0.2 molar copper sulphate was measured into the calorimeter, using a 25cm� pipette. 2. A thermometer was placed in the solution, and the solution was left for one minute to adjust to room temperature. This was timed by a stopwatch. 3. During this time, one gram of zinc was measured out into a small container using electronic scales. After the one minute rest, this was added to the calorimeter and the temperature was taken immediately. 4. The temperature was then taken every 30 seconds, and the mixture was stirred occasionally. The results were recorded in the results table below. For the second experiment, the method was the same as in stages 2, 3 and 4. ...read more.


C = Specific heat capacity of the surroundings ?T = Temperature change Reaction 1 25 x 4.2 x 24 = -2520 J 2520/1000 = -2.52 kJ Reaction 2 25 x 4.2 x 22 = -2310 J 2310/1000 = -2.31 Kj The values are negative because the reactions are exothermic. Conclusion The results suggest that the further apart the results are in the reactivity series, the larger the enthalpy change will be. The results could be further improved in several ways: � The heat loss could be minimalised by placing a plastic lid over the top of the calorimeter � Using a higher grade of equipment. For example, the pipette was grade B, and more accurate results could be achieved by using a higher grade of equipment. � Repeating both experiments and then taking mean values. This would smooth out any anomalous results. It must be understood that the results are only accurate to a certain degree because of the equipment. The scales only weigh to 2 decimal places, and the automatically round up. This means the results could be up to 0.009 figures out. ...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. Electronic spectroscopy - Homoleptic chromium(III) complexes and the spectrochemical series.

    Because chromium(III) is not a d1 system, the spectra of its complexes show more than one d-d transition; however this problem can be more or less overcome by considering the same peak in each spectrum. The ligands investigated by this technique were ethylenediamine (en), acetylacetonate (acac), NH3, Cl- (in the

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

    Where 'X' is one of the five metals. And if X does not react with Copper Sulphate Solution, then we will have: X(s)+ Cu2+(aq)SO42-(aq) � X(s)+ Cu2+(aq)SO42-(aq) Either way the reacting ratios will still be 1:1. So 1 mole of X will react with 1 mole of Copper Sulphate Solution.

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

    This occurs through enzymes (amylase, maltase, peptidases, lipase) changing the substances. The starch is broken down to maltose, which in turn is broken to glucose and transported as sucrose for cellulose or used for energy. The proteins in the seed are converted to polypeptides and then broken to amino acids, which are used for structural or enzyme proteins.

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

    For this reason the solutions were made up into the graduation mark in 10cm3 volumetric flasks. Modifications I was unable to complete this experiment as I ran out of time, thus there are no modifications. After looking at the three preliminary experiments I found that a redox titration between Potassium Manganate (VII)

  1. metal extraction and reactivity

    Extraction of metals from their ores. * Ores are: carbonates, oxides or sulphides of the metal mixed with impurities. * Large lumps of the common ores are first crushed and ground up by very heavy machinery. * Some ores are already concentrated.

  2. Determine the crystallisation temperature of the solution potassium nitrate at different concentrations and use ...

    way to adapt to the experiment because the method I used went easily. Results Volume of water cn R.In cn Crystallisation temperature Reciprocal of absolute temperature 1/T (cm3) (mol dm3) (R = 8.31 Jmol-1 K-1) ( 0C) T(K) (K-1) 8.0 12.36 20.90 62 335 2.98 x 10-3 10.8 9.89 19.04

  1. Reactivity Series Investigation

    without any protective glass whereas the iron and zinc and aluminium didn't react as violent as this because they didn't turn into another sunstance but they did change colour.The end result of the magnesium reacting with oxygen is magnesium oxide that is in word equation magnesium+oxygen equals magnesium oxide.The chemical

  2. Production of Zinc Sulphate

    5. Other zinc salts such as zinc stearate and zinc carbonate are used as preservatives for wood and leather. 6. It is used as raw material for production of lithopone and in synthetic fibre industry. 7. It is used in zinc plating.

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