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5 Cards in this Set
- Front
- Back
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Standard electrode potentials |
All reactions written as reductions. Availability of electrons relative to the hydrogen half cell +ve = less available -> reduced -> oxidising -ve = more available -> oxidised -> reducing |
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Standard hydrogen electrode |
1mol/dm3 H+ in soloution. H(g) at 298K Inert platinum electrode E = 0.00 |
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Other electrodes |
Metal electrode- same as what's in solution Solution = 1mol/dm3 If gas- 100KPa, inert electrode, ions at 1mol/dm3 Or, inert electrode and both ions in same solution at 1mol/dm3 |
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General stuff about voltaic cells |
Half reactions have equilibrium arrows Overall reaction has normal arrow Ions move through salt bridge Electrons move through wire High resistance volt meter to minimise current flow. Cathode = +ve Anode = -ve |
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Gibbs free energy |
Ecell= 0 = spontaneous Ecell =+ve = spontaneous dG = -nFEcell |
