A-Level Chemistry Edexcel 9CH0

understand the terms ‘oxidation’ and ‘reduction’ in terms of electron transfer, applied to s-, p- and d-block elements

be able to predict the thermodynamic feasibility of a reaction using standard electrode potentials

understand that E^θ_cell is directly proportional to the total entropy change and to ln K for a reaction

understand the limitations of predictions made using standard electrode potentials, in terms of kinetic inhibition and departure from standard conditions

know that standard electrode potentials can be listed as an electrochemical series

understand how disproportionation reactions relate to standard electrode potentials

understand the application of electrode potentials to storage cells

understand that the energy released on the reaction of a fuel with oxygen is utilised in a fuel cell to generate a voltage

Knowledge that methanol and other hydrogen-rich fuels are used in fuel cells is expected.

know the electrode reactions that occur in a hydrogen-oxygen fuel cell

Knowledge of hydrogen-oxygen fuel cells with both acidic and alkaline electrolytes is expected.

be able to carry out both structured and non-structured titration calculations including Fe²⁺/MnO₄⁻, and I₂/S₂O₃²⁻

understand the methods used in redox titrations

understand the terms ‘oxidation’ and ‘reduction’ in terms of changes in oxidation number, applied to s-, p- and d-block elements

know what is meant by the term ‘standard electrode potential’, E^θ

know that the standard electrode potential, E^θ, refers to conditions of:

i) 298 K temperature ii) 100 kPa pressure of gases iii) 1.00 mol dm^-3 concentration of ions

know the features of the standard hydrogen electrode and understand why a reference electrode is necessary

understand that different methods are used to measure standard electrode potentials of:

i) metals or non-metals in contact with their ions in aqueous solution ii) ions of the same element with different oxidation numbers

be able to calculate a standard emf, E^θ_cell, by combining two standard electrode potentials

be able to write cell diagrams using the conventional representation of half-cells

understand the importance of the conditions when measuring the electrode potential, E

CORE PRACTICAL 10: Investigating some electrochemical cells

CORE PRACTICAL 11: Redox titration