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

Specific Heat of Copper Lab

Extracts from this document...


J. Ryan Specific Heat of a Metal Pre ? Lab: 1. (mass of water)(specific heat water)(temperature of water final - temperature of water initial)=(mass of metal)(unknown)(temperature of metal final - temperature of metal initial) 2. percentage error = (measure-actual/actual) x 100 Procedure: 1. Measure the initial temperature of the water and the and the metal and also measure the mass of both 2. Measure the mass of the beaker then fill a large beaker which is about half full of water. Place the beaker of water on the hot plate then start heating the water until it reaches boiling point 3) Record the mass of the calorimeter 4) ...read more.


Immediately pour the metal into the calorimeter cup so that the metal is covered by the water. Cover the calorimeter with its cover 9) Insert the thermometer through the small hole in the cover. Stir very slowly with a stirring rod, and record the highest temperature reached by the water. Material Mass Temperature Metal in boiling water 57.39 g ± 0.05 100.8°C± 0.05 Calorimeter 297.86g± 0.05 N/A Calorimeter + water 450.05g± 0.05 17.35°C± 0.05 Water in beaker 152.19± 0.05 100.8°C± 0.05 Water in Calorimeter after hot metal added. 507.44g± 0.05 20.2°C± 0.05 Beaker 177.23g ± 0.05 Follow-Up : X = unknown specific heat of metal (152.19 ± 0.05)(4.186)(20.2 ± 0.05 - 17.35 ± 0.05 ) ...read more.


Another limitation that I think was present was that when we are transferring the metal into the calorimeter the temperature of the metal might have changed a little even thought we tried to move it as quickly as possible and that could be a limitation. There are also some errors that we are not able to prevent from happening. For example, the electrical thermometer could have a different temperature and it will also change the temperature of the water because it will take some time for the temperature to stay at constant. Even though we try as hard to not have any errors human error will always be present. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate 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 International Baccalaureate Chemistry essays

  1. Peer reviewed

    Calculating the specific heat of a metal

    4 star(s)

    heat that was lost by the metal would be the heat gained by the distilled water and the specific heat of the metal could be found, but since heat was lost (this is indicated by the decrease in temperature from 27 to 20 degrees), the maximum heat reached will be

  2. Esterification Equilibrium

    NaOH + HCl HCl -> H+ + Cl- C 0.9531M => V 33.24x10-3 n 0.032 mols 0.032 mols 0.032 mols 0.032 mols 0.032 mols Volume of water = 5 - (0.032x36.45) = 3.83g Calculating uncertainty, Uncertainty = 0.9531 x (33.24x10-3�0.15x10-3)

  1. Chemistry Equilibrium Lab

    the same radius straw with 5mL of water added to cylinder A after results from Table 1. Number of Transfers Volume of Water in a cylinder A (mL � 0.1 mL) Volume of Water in a cylinder B (mL � 0.1 mL)

  2. Effect of Current on The Quantity of Products in Copper Purification Through Electrolysis

    (voir calculs � l'Annexe 2) 3. Pr�parer une premi�re solution de CuSO4 (aq) � un volume de 1000 mL et une concentration de 0,1 mol/L dans la fiole jaug�e de 1000 mL. 4. Pour la pr�paration de solution, garder la m�thode constante en employant le m�me entonnoir pour introduire le

  1. Lab to determine The Specific Heat of a Metal

    Percent Uncertainties Volume of water- (.5 / 100) ? 100 = .5 % Temperature of distilled water- (.5 / 24.2) ? 100 = 2.07% Mass of copper- (.001 / 43.027) ? 100 = .0023% Temperature of copper- (.5 / 95.1)

  2. Electrolysis of copper sulphate

    Paper towels were used to absorb the solution on the cathodes which could have removed a lot of the copper that was deposited on the cathodes post-electrolysis and thus reduced the reading for the change in mass. This could explain why the results obtained in the experiment are low compared to the theoretical results.

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