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

Experiment to find out the enthalpy changes that took place for the reaction between copper sulphate and zinc.

Extracts from this document...

Introduction

Evaluation I conducted an experiment to find out the enthalpy changes that took place for the reaction between copper sulphate and zinc. An enthalpy change of a reaction is the heat exchange with the surroundings at constant pressure. Introduction In this experiment in order to find out the enthalpy change I shall be reacting aqueous copper sulphate with zinc. In this reaction Cu is being reduced and Zn is being oxidised. In this experiment the enthalpy change is exothermic. Enthalpy changes can be both exothermic and endothermic. Exothermic reactions are easily recognised by a rise in temperature. Endothermic reactions require an energy input. Enthalpy is the total energy content of the reacting materials it is given the symbol H. Enthalpy cannot be measured but it is possible to measure enthalpy change when energy is transferred to or from a reaction system. Enthalpy change is given the symbol ?H where ? ...read more.

Middle

?H = 4.18Jg * 50g * 16.5�C = 3448.5J You then need to divide this by the no of moles of zinc used to get the overall enthalpy change. Moles= mass = 2.106 = 0.032 Ar 65.4 3448.5 = 107765 0.032 107765 = 107.77KJ 1000 The overall enthalpy change given out by this experiment is 107.77KJ Limitations and Improvements There were two main limitations in this experiment, mainly the cup and the thermometer. The limitation of the cup was that it was not too well insulated so heat energy was lost more readily to the surroundings. Also there was no top so heat could have escaped through the top. The limitation with the thermometer was the range. By this I mean, when I took a temperature reading the closest I could get was 0.5, i.e. 21.5 31.5. If I had a better range on the thermometer I could get better, more accurate readings. ...read more.

Conclusion

Also I could have had a colorimeter, which could have shown me when the reaction ended. This could have helped me because it would have been a point where I would have recognised when the temperature would start to fall. Another improvement is that I could have done the experiment again and gain another set of results to compare with my original results. Errors and anomalous results. The errors that occurred in this experiment are as follows. When I took a temperature reading my body heat may have interfered with the temperature. Also due to the lack of range on the thermometer I had to use my own guesswork as to what the temperature was when it was between two whole numbers. Also the experiment was not very efficient. By this I mean that a lot of energy was lost to the surrounding as there was a lack of insulation. If you look at my results you will see that there are not any anomalous results. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Organic 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 AS and A Level Organic Chemistry essays

  1. Marked by a teacher

    Reactions of aldehydes and ketones. The purpose of this experiment is to compare ...

    5 star(s)

    , the formation of silver mirror. This reaction is very useful to extinguish aldehyde from ketone as ketone does not show this reaction. Silver mirror formed in a flask The colour of the product mixture after the reaction. 3. Fehling' reagent Aldehydes are also oxidized by the Fehling's solution.

  2. Marked by a teacher

    Experiment to Determine Acidities of Wine. The purpose of this experiment is to ...

    5 star(s)

    Total Acidity Australian Volume of NaOH added (cm3) pH 0 3.2 3 3.3 6 3.4 9 3.4 12 3.5 15 3.6 18 3.7 21 3.8 24 3.8 27 3.9 30 4 33 4.1 36 4.1 39 4.2 42 4.3 45 4.4 48 4.5 51 4.6 54 4.7 57 4.8 60

  1. Preparation of haloalkane. The purpose of this experiment is to prepare 2-chloro-2-methylpropane from ...

    Moreover, although the distillation products were collected from 47oC to 53oC. This does not necessarily mean that the distillation product was purely 2-chloro-2methylpropane. There might be some impurities distilled out together with the product we want.

  2. Determination of the formula of Hydrated Iron (II) Sulphate crystals

    Another procedural uncertainty is the problem with the size of the hydrated iron (II) sulphate crystals used; as the crystals were a relative size, the outside of some of the crystals (depending on how close they were to the heat)

  1. Find the enthalpy change of combustion of a number of alcohol's' so that you ...

    All of this matches with my prediction which proves somewhat that my experiment was a success. There is some further evidence that can explain these findings. There is a certain amount of energy required to break a specific bond, which is related to the bond enthalpy.

  2. Investigating the Enthalpy Changes of Combustion of Alcohols.

    was accurate to 0.1 �C (i.e. has n error of � 0.05 �C), so the percentage error is: 0.1/7.2 x 100 = 1.4% (NOTE: this is a much smaller error that when compared with the normal thermometers. As they measured accurately to only 1 �C, the percentage error would be 14%.

  1. The aim of this experiment is to produce Aspirin. This is an estrification in ...

    * The solution was then titrated with 0.1 mol dm-3 hydrochloric acid. Performing a rough titration A rough titration was carried in order to distinguish an approximate endpoint In order to perform a rough titration a note of the burette reading was recorded to the nearest 0.05cm3.

  2. The aim of this experiment is to investigate the enthalpy change of combustion for ...

    value and the calculated value is going to be a lot greater than that calculated from graph one. %Error = -486 - -245 x 100 -486 =-241 x100 -486 =49.6% This value is dramatically larger, but this was expected due to error noted in the experiment involving the copper calorimeter.

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