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

Chemistry Lab- Determining enthalpy change of a reaction. Adding zinc to copper sulfate resulted in a displacement reaction that created copper metal to precipitate as a solid.

Extracts from this document...

Introduction

Name: Laraib Hussain Class: IB 1 Chemistry Lab: Experiment 22 - Determining an enthalpy change of reaction Exp.22 Determining the Enthalpy Change of a reaction Data Collection Quantitative Data - Table of Results: Trial 1 Mass of filter paper: 1.50 � 0.01 g Mass of zinc + filter paper: 7.52 � 0.01 g Trial 2 Mass of filter paper: 1.49 � 0.01 g Mass of zinc + filter paper: 7.58 � 0.01 g Time (� 0.01s) Temperature (� 0.5�C) Time (� 0.01s) Temperature (� 0.5�C) 0.00 24.0 0.00 25.0 30.00 24.0 30.00 25.0 60.00 24.0 60.00 25.0 90.00 23.5 90.00 25.0 120.00 23.5 120.00 25.0 150.00 23.5 150.00 25.0 Addition of Zinc Powder at 3 minutes, then temp. recorded for additional 6 minutes Addition of Zinc Powder at 3 minutes, then temp. ...read more.

Middle

- (Mass of filter paper) = (7.52 � 0.01 g) - (1.50 � 0.01 g) = (7.52 - 1.50) � (0.01 + 0.01) = 6.02 � 0.02 g 2. To Calculate the Enthalpy Change (? H) of the reaction we will use the formula: Where m = mass of solution (g) c = specific heat capacity of water: 4.18 ?T = rise in temperature (� C) Note: We assumed that the products in the reaction have the same specific heat capacity as water. Also we assume that the reactants have a density of 1g hence the mass of the reactants will be: Mass = density � volume = 1g � 25 = 25 g Total mass of solution = (6.02 � 0.02 g) + 25 g = 31.02 g �0.02 The rise in temperature (?T) ...read more.

Conclusion

The limiting reagent is CuSO4. No. of moles of CuSO4 = concentration � volume = 1 mol dm-3 � (25cm3 � 1000cm3) = 1 � 0.025 dm3 = 0.025 moles 6. Hence, the Enthalpy Change of 1 mole of Zn and CuSO4: ?H = = Measurement: -3.8 � 0.025 = -152 KJ mol-1 Relative error: 0.1 � -3.8 = -0.02631578947 Absolute Uncertainty: -0.02631578947 � -152 = � 4 Final Answer: -152KJ mol-1 � 4 ?H of this reaction is -152 KJmol-1 � 4 7. Percentage error= � 100% Literature value of Enthalpy Change for this reaction is -217KJmol-1 = � 100% = [-217 - (- 152 �4)] �100% -217 = (-65�4) �100% -217 Measurement: -65� -217= - 0.2995391705 Relative error: (4� -65) �100= - 6.153846154 % Absolute uncertainty: - 0.2995391705 � - 6.153846154 % = � 0.018 � �0.02 Final answer: (- 0.30 � 0.02) � 100 = - 30 % � 2 ...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)

    What can be concluded is that the heat that is absorbed is the heat being released.

  2. The Enthalpy of Neutralization

    Our equipment throughout the experiment was basic in nature, made for a high school chemistry laboratory and was not as precise as it could have been if we had been aiming for prime results. Our volumes had an uncertainty of plus/minus 0.5ml which gave us a constant 2% absolute error

  1. Acids/Bases Design Lab. How does a change in the pH value of a solution ...

    This beaker was labeled 'Beaker BT1', and a mercury thermometer was inserted inside the solution, and the temperature was recorded. 7. A clean, and dry weighing boat was placed on the electronic milligram balance (+/- 0.001g), and its mass was recorded to the nearest 0.001g.

  2. Thermodynamics: Enthalpy of Neutralization and Calorimetry

    g 76.028 g Mass of Metal Cylinder 17.715 g 17.771 g 17.751 g Mass of Cold Water 69.133 �.001 g 67.634 �.001 g 68.240 �.001 g 68.336 �.001 g Temperature of Cold Water 21.7 �.5 C� 21.3 �.5 C� 22.0 �.5 C� Temperate of Cylinder 97.1 �.5 C� 95.3 �.5

  1. Electrolysis of copper sulphate

    1. Fourth current reading is 0.8 amps. Total Quantity of charge = Current Ax TimeS â 0.8 x 120 = 96 Coulombs 1. To find number of electrons transferred. Number of e- =Total Quantity of ChargeCharge of 1e- â961.60217733x10-19= 6 x1020electrons 1.

  2. IA-Enthalpy Change of Reaction - Zinc and Copper Sulphate.

    Repeat steps 2 to 7 four more times. II. Data Collection and Processing Quantitative Data Example Calculation: Finding the Final and Initial Tempeartures Step 1. Find the linear fit model of the graph The linear fit model of f(x)=-0.03028x+70.95 can be gained from the graph above.

  1. Chemistry Lab Report- Determining the Enthalpy of Enthalpy Change, H, for a Redox Reaction ...

    Number of Moles (Cu + Zn2+) = Mass/Mr Mass=Mass of CuSO4 Solution (g) (±0.05g) + Mass of Zinc Powder (g) (±0.05g) Mass= 25.0g (±0.05g) +4.0g (±0.05g) Mass= 29.0g (±0.05g) Convert to Kg: 29.0g/1000= 0.0290Kg Mr= Cu-1; 63.55 x 1=63.55 S-1; 32.06 x 1=32.06 O-4 16.00 x 4=64.00 Total relative mass

  2. The aim of this experiment is to examine the enthalpy of combustion of the ...

    + 712 O2 (g) 5 CO2 (g) + 6 H2O (g) The same formulas have to be used for these calculations. Because in this reaction heat energy is transformet to water, in order to do the calculations,we must know the heat energy that has been given out.

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