Measurement of an Enthalpy Change (Oxford AQA International A Level Chemistry)

Revision Note

Alexandra Brennan

Written by: Alexandra Brennan

Reviewed by: Stewart Hird

Required Practical 2: Measuring Enthalpy Change

Objective

To determine the enthalpy change for the conversion of anhydrous copper(II) sulfate into hydrated copper(II) sulfate, ΔH3

This enthalpy change cannot be measured directly but can be calculated from:

  • The enthalpy change for the conversion of anhydrous copper sulfate to copper sulfate solution, ΔH1

  • The enthalpy change for the conversion of hydrate copper sulfate to copper sulfate solution, ΔH2

cycle-cuso4

Apparatus

  • Hydrated copper(II) sulfate crystals

  • Anhydrous copper(II) sulfate powder

  • Polystyrene cups with lids

  • 250 cm3 for holding polystyrene cup

  • Stand and clamp

  • Thermometer

  • 25 cm3 measuring cylinders x 2

  • Weighing bottles x 2

  • Stopwatch

  • Graph paper

  • Stirrer

  • Distilled water

  • Digital balance

Method

Experiment 1: Determining ΔH1

  1. Weigh out between 3.90 g and 4.10 g of anhydrous copper(II) sulfate in a weighing bottle and record the mass

  2. Measure 25 cm3 of deionised water into a polystyrene cup using a measuring cylinder

  3. Record its temperature at the beginning (t=0)

  4. Start the timer and record the temperature every minute for a further three minutes

  5. At the fourth minute, add the powdered anhydrous copper(II) sulfate rapidly to the polystyrene cup and continue to stir, but do not record the temperature.

  6. At the fifth minute and for every minute up to 15 minutes, stir and record the temperature of the solution in the polystyrene cup.

Experiment 2: Determining ΔH2

  1. Weigh out between 6.20 g and 6.30 g of hydrated copper(II) sulfate in a weighing bottle and record the mass

  2. Measure 24 cm3 of deionised water into a polystyrene cup using a measuring cylinder

  3. Record its temperature at the beginning (t=0)

  4. Start the timer and record the temperature every minute for a further three minutes

  5. At the fourth minute, add the powdered hydrated copper(II) sulfate rapidly to the polystyrene cup and continue to stir, but do not record the temperature.

  6. At the fifth minute and for every minute up to 15 minutes, stir and record the temperature of the solution in the polystyrene cup.

How to set up your equipment

How to set up your equipment for calorimetry

Practical Tip

Be careful not to get the anhydrous copper(II) on your skin as it can cause irritation.

Results

Record your results in a table like this:

Temperature / oC

Experiment 1

Experiment 2

0

1

2

3

4

x

x

5

6

7

8

9

10

11

12

13

14

15

The temperature is not recorded at minute 4 as this is when you have added the hydrated / anhydrous copper(II) sulfate.

Evaluation

For each set of results:

  1. Plot a graph of temperature (on the y-axis) against time (on the x-axis)

  2. Draw two separate best fit lines; one, which joins the points before the addition of hydrated / anhydrous copper(II) sulfate, and one which joins the points after the addition

  3. Extrapolate both lines to the fourth minute

  4. Use your graph to determine the temperature change at the fourth minute

  5. Use q = m x c x ΔT and ΔH = q/ n to determine ΔH1 and ΔH2

  6. Determine the enthalpy change for ΔH3 using:

    ΔH3 = ΔH1 – ΔH2

    cycle-cuso4

Worked Example

A student obtained the data in Table 1 by carrying out the methods above.

They added 4.94 g anhydrous copper(II) sulfate in experiment 1.

They added 7.72 g hydrated copper(II) sulfate in experiment 2.

Table 1

Temperature / oC

Experiment 1

Experiment 2

0

19.8

19.6

1

19.8

19.8

2

19.8

19.8

3

19.8

19.8

4

x

x

5

27.8

18.2

6

27.7

18.2

7

27.6

18.2

8

27.6

18.2

9

27.5

18.2

10

27.5

18.2

11

27.4

18.2

12

27.3

18.2

13

27.2

18.2

14

27.0

18.2

15

26.8

18.2

Question

  1. Plot a graph of each set of results to determine the temperature change for each reaction

  2. Calculate the enthalpy change for each reaction, ΔH

  3. Calculate the enthalpy change, in kJ mol –1 for the hydration of copper(II) sulfate.

The specific heat capacity of water is 4.2 J/kg°C.

Answer:

  1. The graphs for each set of results and temperature changes are:

    Experiment 1: Addition of anhydrous copper(II) sulfate

    Enthalpy change for anhydrous copper sulfate

    The temperature change is 8.4 oC

    Experiment 2: Addition of hydrated copper(II) sulfate

    enthalpy change hydrated copper sulfate

    The temperature change is 1.7oC

  2. The enthalpy change for each reaction:

    Experiment 1:

    • q = m x c x ΔT

    • q= 25 x 4.2 x 8.4 = 882 J = 0.882 kJ

    • n= 4.94 / 159.6 = 0.0310 mol

    • ΔH1 = q / n = 0.882 / 0.0310 = -28.45 kJ mol-1

    Experiment 2:

    • q = m x c x ΔT

    • q= 25 x 4.2 x 1.7 = 178.5 J = -0.1785 kJ

    • n= 7.72 / 249.6 = 0.309

    • ΔH2 = q / n = 0.1785 / 0.309= +5.78 kJ mol-1

  3. The enthalpy change, in kJ mol –1 for the hydration of copper(II) sulfate is:

    ΔH3 = ΔH1 – ΔH2

    ΔH3 = -28.45 -(+5.78 ) = -34.2 kJ mol-1

Examiner Tips and Tricks

Remember: The mass of the water would be 25 g as 25 cm3 of water is used and the density of water is 1 g cm-3.

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Alexandra Brennan

Author: Alexandra Brennan

Expertise: Chemistry

Alex studied Biochemistry at Newcastle University before embarking upon a career in teaching. With nearly 10 years of teaching experience, Alex has had several roles including Chemistry/Science Teacher, Head of Science and Examiner for AQA and Edexcel. Alex’s passion for creating engaging content that enables students to succeed in exams drove her to pursue a career outside of the classroom at SME.

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.