EMF of Electrochemical Cells (Oxford AQA International A Level Chemistry)

Revision Note

Richard Boole

Written by: Richard Boole

Reviewed by: Stewart Hird

Required Practical 8: Measuring EMF

Objective

Measure the electromotive force (EMF) of an electrochemical cell.

Apparatus

  • Copper and zinc foil pieces

  • Propanone

  • 2.0 mol dm–3 NaCl solution

  • 1.0 mol dm–3 CuSO4 solution

  • 1.0 mol dm–3 ZnSO4 solution

  • Sandpaper

  • Cotton wool

  • 100 cm3 beakers

  • Plastic / glass U-tube

  • High resistance voltmeter

  • Two wires and crocodile clips

  • Metal samples

Method - Setting up a standard cell

  1. Take one piece of copper and one piece of zinc:

    • Clean them using sandpaper

    • Degrease the metal using cotton wool and propanone.

  2. Place the copper into a 100 cm3 beaker with 50 cm3 of 1 mol dm–3 CuSO4 solution

  3. Place the zinc into a 100 cm3 beaker with 50 cm3 of 1 mol dm–3 ZnSO4 solution

  4. Prepare the salt bridge:

    • Plug one end of the plastic / glass U-tube with cotton wool

    • Fill the plastic / glass U-tube with 2 mol dm–3 NaCl solution

    • Plug the free end of the tube with cotton wool which has been soaked in 2 mol dm–3 NaCl solution

  5. Connect the two beakers with the inverted U-tube so that the plugged ends are in the separate beakers.

  6. Connect the Cu (s) | Cu2+ (aq) and Zn (s) | Zn2+ (aq) half-cells:

    • Using a crocodile clip, connect a wire to the piece of copper

    • Plug the other end of this wire into the high resistance voltmeter

    • Using a crocodile clip, connect a wire to the piece of zinc

    • Plug the other end of this wire into the high resistance voltmeter

  7. Read off the voltage

Diagram

Diagram of equipment needed to calculate electromotive force

Practical Tip

  • If you set up another cell, replace the salt bridge to prevent cross contamination of ions between half cells

Evaluation

  • Write the conventional representation for the cell that you have constructed

  • You may be asked to explain why the value you recorded is different to the theoretical value

Worked Example

The half-equations and standard electrode potential values for cell constructed during this required practical are:

Zn2+ (aq) + 2e- ⇌ Zn (s)       E = -0.76 V

Cu2+ (aq) + 2e- ⇌ Cu (s)       E = +0.34 V

  1. Write the conventional representation for the cell constructed in this required practical.

  2. Explain why the EMF value recorded is different to the theoretical value.

Answers:

  1. The conventional representation for the cell constructed in this required practical is:

    1. The Cu2+ / Cu cell has the higher E value

    2. Therefore, this is the reduction reaction which is on the right hand side of the electrochemical cell

    3. The Zn2+ / Zn cell has the lower E value

    4. Therefore, this is the oxidation reaction which is on the left hand side of the electrochemical cell

    5. So, the conventional representation is:

Zn (s) | Zn2+ (aq) || Cu2+ (aq) | Cu (s)

  1. The EMF value recorded is different to the theoretical value because:

    • The electrochemical cell is not operating under standard conditions

Method - Measuring comparative electrode potentials of different metals

  1. Clean a piece of copper using sandpaper

  2. Using a crocodile clip, connect a wire to the piece of copper

  3. Plug the other end of this wire into the high resistance voltmeter

  4. Prepare the salt bridge:

    • Cut a piece of filter paper to about the same area as the copper

    • Wet the filter paper with the sodium chloride solution

    • Place this on top of the copper

  5. Preparing the metal sample:

    • Connect a second wire lead to the voltmeter

    • Connect a crocodile clip to the other end of the wire

    • Place a piece of sample metal in the crocodile clip

  6. Testing the metal sample

    • Hold the sample metal against the filter paper

    • Record the voltage and sign in a suitable table

    • Repeat this process with different metal samples

Diagram

Equipment for measuring comparative electrode potentials of different metals

Practical Tip

  • If you don't get a positive reading on the voltmeter swap the terminals around

  • Voltmeters will have marked positive and negative terminals (usually in red and black, respectively), so when you get a positive reading this tells you the relative polarity of the metals in the cell

Results - Measuring comparative electrode potentials of different metals

  • Record your results for each test carefully in a suitable table like the one below: 

Sample metal electrode

EMF / V

Zinc

Iron

Silver

Nickel

Evaluation

  • The half-equation and E value for copper are:

Cu2+ (aq) + 2e- → Cu (s)              E = +0.34 V

  • Use this information and your results to determine the E values for the sample metals

  • Suggest how you could construct the cell with the largest electromotive force from the sample metals

Worked Example

An electrochemical cell is constructed using:

  • A Cu / Cu2+ half-cell

  • An appropriate half-cell using zinc, iron, silver or nickel

The electromotive force produced in each cell is recorded in the table below.

Sample metal

EMF / V

E / V

Zinc

+1.10 V

Iron

+0.78 V

Silver

+0.46 V

Nickel

+0.60 V

Cu2+ ions were reduced to Cu atoms when paired with zinc, iron and nickel half-cells.

The half-equation and E value for copper are:

Cu2+ (aq) + 2e- → Cu (s)              E = +0.34 V

Ag+ ions were reduced to Ag atoms when paired with the copper half-cell.

  1. Complete the table by deducing the E value for each sample metal.

  2. Suggest how you could construct the cell with the largest electromotive force from the sample metals.

  3. Calculate the electromotive force for the cell with the largest electromotive force from the sample metals.

Answers: 

  1. Deducing E value for each sample metal:

    • Ecell = Ereduction - Eoxidation

    • Zinc

      • Cu2+ ions were reduced

      • (+1.10) = (+0.34) - Eoxidation

      • Eoxidation = (+0.34) - (+1.10) = -0.76 V

    • Iron

      • Cu2+ ions were reduced

      • (+0.78) = (+0.34) - Eoxidation

      • Eoxidation = (+0.34) - (+0.78) = -0.44 V

    • Silver

      • Ag+ ions were reduced

      • (+0.46) = Ereduction - (+0.34)

      • Ereduction = (+0.46) + (+0.34) = +0.80 V

    • Nickel

      • Cu2+ ions were reduced

      • (+0.60) = (+0.34) - Eoxidation

      • Eoxidation = (+0.34) - (+0.60) = -0.26 V

    • So, the completed table is:

Sample metal

EMF / V

E / V

Zinc

+1.10 V

-0.76

Iron

+0.78 V

-0.44

Silver

+0.46 V

+0.80

Nickel

+0.60 V

-0.26

  1. To construct the cell with the largest electromotive force from the sample metals:

    • This requires the half-cells with the highest and lowest E values

      • Highest E value: Ag / Ag+ with a value of +0.80 V

      • Lowest E value: Zn / Zn2+ with a value of -0.76 V

    • The Ag / Ag+ half-cell requires:

      • A silver electrode

      • A 1.0 mol dm-3 solution of Ag+ ions

    • The Zn / Zn2+ half-cell requires:

      • A zinc electrode

      • A 1.0 mol dm-3 solution of Zn2+ ions

    • The half-cells are connected with:

      • A high resistance voltmeter

      • A suitable salt bridge

  2. The electromotive force for the cell with the largest electromotive force from the sample metals is:

    • Ag / Ag+ has the highest (most positive) E value, which means that this is the reduction reaction

    • Ecell = Ereduction - Eoxidation

    • Ecell = (+0.80) - (-0.76) = +1.56 V

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Richard Boole

Author: Richard Boole

Expertise: Chemistry

Richard has taught Chemistry for over 15 years as well as working as a science tutor, examiner, content creator and author. He wasn’t the greatest at exams and only discovered how to revise in his final year at university. That knowledge made him want to help students learn how to revise, challenge them to think about what they actually know and hopefully succeed; so here he is, happily, 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.