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Che Trial Amali f5 c1

This document provides information about redox equilibrium and the Daniell cell. It discusses how the voltage of the Daniell cell is determined by the difference between the standard electrode potentials of the cathode and anode. Specifically, it states that the voltage is equal to the potential of the cathode minus the potential of the anode. It then gives an example calculation for the Daniell cell using copper and zinc electrodes in copper and zinc salt solutions.

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Lo Hilary
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180 views1 page

Che Trial Amali f5 c1

This document provides information about redox equilibrium and the Daniell cell. It discusses how the voltage of the Daniell cell is determined by the difference between the standard electrode potentials of the cathode and anode. Specifically, it states that the voltage is equal to the potential of the cathode minus the potential of the anode. It then gives an example calculation for the Daniell cell using copper and zinc electrodes in copper and zinc salt solutions.

Uploaded by

Lo Hilary
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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Redox Equilibrium Chapter 1

• Cell notation for a Daniell cell:


Zn(s) │ Zn2+(aq, 1.0 mol dm–3) ║ Cu2+(aq, 1.0 mol dm–3) │ Cu(s)

Anode (negative terminal) Cathode (positive terminal)

• The voltage reading, E cell for the Daniell cell:


0
The cell voltage, E0cell can be determined
E0cell = E0(cathode) – E0(anode) by using the following formula:
E0cell = (+0.34) – (- 0.76) = + 1.10 V E0cell = E0(positive terminal) – E0(negative terminal)
E0cell = E0(cathode) – E0(anode)

1A Determining the Voltage of a Voltaic Cell


Learning Science
Aim: To determine the voltage of a voltaic cell by using different pairs of metals. PAK 21 Through Inquiry
Problem statement: How can different pairs of metals dipped into electrolytes affect the
voltage of the voltaic cell?
Hypothesis: The greater the difference of the value of standard electrode potential of pairs
of metals, the greater the voltage reading.
Variables:
(a) Manipulated variables : Different pairs of metals.
(b) Responding variables : The voltage reading of the cell.
(c) Fixed variables : Volume and concentration of electrolytes.
Operational definition – Chemical cell: Voltmeter shows a reading when different types of pairs
of metals are dipped into electrolytes.
Materials: State a list of different metal plates and suitable salt solutions with a concentration of
1.0 mol dm−3.
Apparatus: Sandpaper, voltmeter and connecting wire with crocodile clips and state a suitable
apparatus to construct a chemical cell.
Procedure:
1. Using the provided metal plates and salt solutions, plan an experiment to construct
a simple chemical cell or a chemical cell that combines two half-cells.
2. Draw a labelled diagram of a simple chemical cell or a chemical cell that combines two half-cells
to carry out this experiment.
3. Write the investigation steps clearly.
4. Record all observations.
Results:
Record all observations in the following table.
Pair of metals Voltage (V) Negative terminal(anode) Positive terminal (cathode)

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