EMF of Electrochemical Cells (Oxford AQA International A Level Chemistry)
Revision Note
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
Take one piece of copper and one piece of zinc:
Clean them using sandpaper
Degrease the metal using cotton wool and propanone.
Place the copper into a 100 cm3 beaker with 50 cm3 of 1 mol dm–3 CuSO4 solution
Place the zinc into a 100 cm3 beaker with 50 cm3 of 1 mol dm–3 ZnSO4 solution
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
Connect the two beakers with the inverted U-tube so that the plugged ends are in the separate beakers.
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
Read off the voltage
Diagram
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) Eꝋ = -0.76 V
Cu2+ (aq) + 2e- ⇌ Cu (s) Eꝋ = +0.34 V
Write the conventional representation for the cell constructed in this required practical.
Explain why the EMF value recorded is different to the theoretical value.
Answers:
The conventional representation for the cell constructed in this required practical is:
The Cu2+ / Cu cell has the higher Eꝋ value
Therefore, this is the reduction reaction which is on the right hand side of the electrochemical cell
The Zn2+ / Zn cell has the lower Eꝋ value
Therefore, this is the oxidation reaction which is on the left hand side of the electrochemical cell
So, the conventional representation is:
Zn (s) | Zn2+ (aq) || Cu2+ (aq) | Cu (s)
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
Clean a piece of copper using sandpaper
Using a crocodile clip, connect a wire to the piece of copper
Plug the other end of this wire into the high resistance voltmeter
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
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
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
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 Eꝋ value for copper are:
Cu2+ (aq) + 2e- → Cu (s) Eꝋ = +0.34 V
Use this information and your results to determine the Eꝋ 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 | Eꝋ / 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 Eꝋ value for copper are:
Cu2+ (aq) + 2e- → Cu (s) Eꝋ = +0.34 V
Ag+ ions were reduced to Ag atoms when paired with the copper half-cell.
Complete the table by deducing the Eꝋ value for each sample metal.
Suggest how you could construct the cell with the largest electromotive force from the sample metals.
Calculate the electromotive force for the cell with the largest electromotive force from the sample metals.
Answers:
Deducing Eꝋ value for each sample metal:
Ecellꝋ = Ereductionꝋ - Eoxidationꝋ
Zinc
Cu2+ ions were reduced
(+1.10) = (+0.34) - Eoxidationꝋ
Eoxidationꝋ = (+0.34) - (+1.10) = -0.76 V
Iron
Cu2+ ions were reduced
(+0.78) = (+0.34) - Eoxidationꝋ
Eoxidationꝋ = (+0.34) - (+0.78) = -0.44 V
Silver
Ag+ ions were reduced
(+0.46) = Ereductionꝋ - (+0.34)
Ereductionꝋ = (+0.46) + (+0.34) = +0.80 V
Nickel
Cu2+ ions were reduced
(+0.60) = (+0.34) - Eoxidationꝋ
Eoxidationꝋ = (+0.34) - (+0.60) = -0.26 V
So, the completed table is:
Sample metal | EMF / V | Eꝋ / 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 |
To construct the cell with the largest electromotive force from the sample metals:
This requires the half-cells with the highest and lowest Eꝋ values
Highest Eꝋ value: Ag / Ag+ with a value of +0.80 V
Lowest Eꝋ 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
The electromotive force for the cell with the largest electromotive force from the sample metals is:
Ag / Ag+ has the highest (most positive) Eꝋ value, which means that this is the reduction reaction
Ecellꝋ = Ereductionꝋ - Eoxidationꝋ
Ecellꝋ = (+0.80) - (-0.76) = +1.56 V
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