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

Enthalpy change of a displacement reaction

Extracts from this document...


Chemistry TAS Report 1. Experiment Number : 4 2. Date : 15/10/07 3. Title : Enthalpy change of a displacement reaction 4. Aims/Objective : To determine the enthalpy change of a displacement reaction (Between zinc and copper (II) ions) 5. Introduction : Excess zinc powder is added in a measured amount of aqueous copper (II) sulphate. The temperature change is then measured over a period of time so the enthalpy of this reaction can be calculated. 6. Relevant Equations/Chemical Reactions Involved : Zn (s) + CuSO4(aq) ?? ZnSO4(aq) + Cu(s) 7. Chemicals : 1.00M copper (II) sulphate solution 25.0 cm3 Zinc powder (in excess) 5.9g 8. Apparatus and equipment : Safety spectacle x 1 Spatula x 1 25 cm3 pipette x 1 Balance x 1 Pipette filler x 1 Thermometer(0-100 oC) ...read more.


sulphate solution was pipetted into a polystyrene cup. 4. Thermometer was put through the hole of the lid. The solution was stirred continuously and the temperature was recorded every half minute for 6 minutes. 10. Observation : The blue colour of the solution disappears. Brown solid is formed. Some zinc powder remains there. 11. Data, Calculation and Results : a. Results Table Time/min 0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 4.5 Temperature/oC 25.0 25.0 25.0 25.0 25.0 25.0 25.0 60.0 73.0 71.0 Time/min 5.0 5.5 6.0 6.5 7.0 7.5 8.0 8.5 9.0 9.5 Temperature/oC 69.0 68.0 67.0 65.5 64.5 63.5 62.5 61.5 60 59 b. Calculations 1&2. ...read more.


?? ZnSO4(aq) + Cu(s) ?H = - 221 kJ mol-1 12. Conclusion : It was found that the enthalpy change of a displacement reaction (Between zinc and copper (II) ions) was - 221 kJ mol-1. 13. Answer to questions 1. % error = {[- 221 - (- 217)]/- 217 }x 100% = 1.84% The experimental value is more negative than the accepted value. 2. Reasons : (1) Heat is lost to the surrounding. (2) The specific heat capacity of the solution is not the same as that of water. 3. CuSO4 is not in excess which is used up totally. No matter that more zinc is used or powder is very finely divided, same amount of the solution is used so there is same increase in temperature. ...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 Physical 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 Physical Chemistry essays

  1. Investigating the Rate of the Reaction between Bromide and Bromate Ions in Acid Solution

    Nickel (II) Iron (III) Manganese (II) (Table 2.7.3) I can compare the rates of reaction with each catalyst by comparing the values of , since this is proportional to rate. The higher the value of , the faster the rate of reaction. I will analyse the results of varying the temperature using a catalyst in exactly the same

  2. Double Displacement Reactions

    ii. Complete the following for each solution: iii. Take one to two drops of the solution and place it in all the boxes which are marked on your grid transparency. iv. After all solutions have been combined, write in your data chart whether a precipitant has formed, and if so, describe the precipitant; describe the composition of the solution.

  1. Explain what is meant by the following terms: i) Oxidising agent: ii) Displacement reaction: ...

    Displacement reaction: In simple terms a displacement reaction is what it states it is. An element- (strictly speaking an ion), within a compound is literally displaced from that compound within a reaction, and is replaced (displaced) by another (more reactive)

  2. Investigating the rate of reaction between peroxydisulphate(VI) ions and iodide ions

    By taking the natural log of the Arrhenius equation, a linear equation can be formed. Therefore this allows a graph of 1/T against. lnk to be drawn. The gradient of this graph (m) will therefore be the negative activation enthalpy (EA)

  1. Investigating how concentration affects rate of reaction

    Whilst conducting this pre-test I used a magnetic stirrer. However, I was not sure whether this was the most appropriate method to use. To solve this I conducted another pre-test, which is shown in the table below: Concentration of Potassium Bromide (mol/dm-3) Time Taken When Stirred by Hand (seconds)

  2. Individual investigation - Reaction to be studied Rate of reaction between propanone and ...

    0.105 0.035 0 270 0.100 0.025 0 300 0.090 0.020 0 330 0.090 0.010 0 360 0.085 0.005 0 AS shown in the calculation, I found the rate of all reactants. RATE/ S-1 � ( 10-4) Concentration/moldm-3 -5.33 0.001 -5.70 0.002 -4.76 0.004 For iodine: For HCL: RATE/ S-1 � ( 10-4)

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