• 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

# 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

# Related AS and A Level Organic Chemistry essays

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

5 star(s)

and the water=H2O should be hypohalic acid=HXO): If a methyl ketone is present, it reacts with the hypohalite in a three-step process: (1) R-CO-CH3 + 3 OX- � R-CO-CX3 + 3 OH- (2) R-CO-CX3 + OH- � RCOOH + -CX3 (3)

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

5 star(s)

98 10.3 Calculations Calculating the Total Acidity of Each Wine Australian As can be seen from the results, it took 89cm3 to bring the wine to the equivalence point of pH 8.2. The number of moles of NaOH needed for this is given by: Tartaric acid is now used as our representative acid in the wine.

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

189.87 188.34 1.53 17.5 37.5 20 Butan-1-ol Trial 2 200 124.45 121.46 2.99 17.5 37.5 20 Butan-1-ol Trial 3 200 211.39 209.63 1.76 16 36 20 I am going to use the following formula to work out how much energy in form of heat was transferred to the water in

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

8.45 cm3 8.40 cm3 Concordant results 8.45 cm3 8.40 cm3 Mass of aspirin used = 1.5067g Weight of container = 0.0000g Preparation of Aspirin (12) Calculating the percentage yield % yield = actual yield x 100 Theoretical yield Mr of salicylic acid = C7H603 12 x 7 + 1 x

2. ## Comparing the enthalpy changes of combustion of different alcohols

This creates a dipole charge in which the partially positive carbon atom joined to the Hydroxyl group is stabilised by the effect of two neighbouring methyl groups. The increase in Enthalpy change of combustion for each fuel is due to the amount of bonds available for the atom to make with Oxygen in its combustion.

1. ## Investigating the Enthalpy Changes of Combustion of Alcohols.

There is, undoubtedly, a pattern in the results gathered. This would suggest that my experiment was not as through as the procedures used to measure the enthalpy of combustion for data banks like Data Sheets: Table 17 (2) (Appendix A).

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

From finding the gradient of the results found in the data book I determined that the most accurate result for the enthalpy change of combustion per carbon atom is -600KJ/mol per carbon atom in the chain length. This shows that even the bond energy calculations are not entirely accurate, as

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