• 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. Rates of Reaction Lab

    Volume of HCl Using the same measuring cylinder to minimize uncertainties Reading the graduation properly- noting the meniscus at the exactly 20 ml Controlled stirring Stirring can be controlled by using a magnetic stirrer. Apparatus and Raw Materials * Stopwatch * Clamp stand * Delivery tube * 100ml Gas syringe

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

    The water was then decanted from the 50cm3 beaker into a waste beaker. 12. The beaker, labeled BRT1, containing the recently rinsed zinc metal strip that reacted with the hydrochloric acid solution for one minute, was then placed on a hot plate set to low heat, and allowed to dry off for 5 minutes.

  1. IB chemistry revision notes

    The step increases on the energy change increases as we get closer to the nucleus. Tips for drawing: * The electronic structure backwards * Each "flat" set gets slightly steeper each time. * The "steps" get slightly bigger each time.

  2. The Enthalpy of Neutralization

    This could be due to a number of reasons, including our equipment's precision, some uncontrolled variables (room temperature, human contact with the container) and random error such as misreading of the volume of solutions or thermometer's display ( caused by parallax).

  1. 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.

  2. 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

  1. Electrolysis of copper sulphate

    Reaction at the cathode: Cu2+ + 2e- â Cu ∴moles of Cu= moleselectrons2â 0.00024870466322= 0.00037375415 moles 1. To find Mass of Cu mass = moles x Molar Mass = 0.001243523316 x 63.5 = 0.024 g of Cu deposited (2.s.f) 1.

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

    This increase is attributed to the fact there is 1 more C-C bond and 2 more C-H bonds broken each time, which means the burning of the fuel is more exothermic so more heat will be given out to the surroundings and the enthalpy change will be greater.

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