Applications and skills:
- Calculation of cell potentials using standard electrode potentials.
- Prediction of whether a reaction is spontaneous or not using Eo values.
- Determination of standard free-energy changes (∆Go) using standard electrode potentials.
- Explanation of the products formed during the electrolysis of aqueous solutions.
- Perform lab experiments that could include single replacement reactions in aqueous solutions.
- Determination of the relative amounts of products formed during electrolytic processes.
- Explanation of the process of electroplating.
Guidance:
- Electrolytic processes to be covered in theory should include the electrolysis of aqueous solutions (eg sodium chloride, copper(II) sulfate etc) and water using both inert platinum or graphite electrodes and copper electrodes. Explanations should refer to Eº values, nature of the electrode and concentration of the electrolyte.
- ∆G° = -nFE°is given in the data booklet in section 1.
- Faraday’s constant = 96 500 C mol-1 is given in the data booklet in section 2.
- The term “cells in series” should be understood.
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- Topic 15.2—spontaneity of a reaction
- Option C.6—Nernst equation
- Biology option B.3—environmental protection; waste treatment and microbial fuel cells
Aims:
- Aim 8: Biological fuel cells can produce electrical energy to power electrical devices, houses, factories etc. They can assist in environmental clean-up. Microbial fuel cells (MFCs) powered by microbes in sewage can clean up sewage which may result in cost-free waste water treatment.
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