Topic 14
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What is the procedure to set up an electrochemical cell
Clean metals with sandpaper to remove impurities Wash metal surface with propanone Place each element into a solution containing the ion of the same metal Make the salt bridge from filter paper soaked in KNO3 and link each 2 beakers Connect the electrodes with wires, crocodile clips and a voltmeter
Why is platinum a good electrode
Electrically conductive and inert
What happens to the electrode(half cell) when it has been reduced in a redox reaction
Reduction means the half cell has gained electrons so the electrode will get thicker
What is the salt bridge and it’s purpose
Salt bridge is filter paper with saturated KNO3 solution. Completes the circuit Allows ions to flow through which balances the charges
What is the voltage of the Standard hydrogen electrode
0V
What happens to a half cell when it has been oxidised in a redox reaction
The electrode will become thinner when more of the metal ion is produced
What are the standard conditions for the standard hydrogen electrode
Temperature at 298K Pressure at 100Kpa Concentrations of ions at 1mol/dm³
What affects the potential value of a half cell
Temperature Concentration Pressure
If a reaction is feasible is the E cell value positive or negative
Positive
When is a Platinum electrode used in an electrochemical half cell What is the solution
When there is no suitable Metal solid available to act as an electrode And this means when The oxidation/ ionic equation only includes ions Mn³+ e- —→ Mn²+ Since there is no Solid Mn in the ionic equation Platinum is the electrode Solution contains both Mn²+ and Mn³+ ions