Book: UTS: 21 Flashcards
The meanings of oxidation and reduction; why an oxidizing agent is reduced and a reducing agent is oxidized.
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How the half-reaction method is used to balance redox reactions in acidic or basic solution.
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The distinction between voltaic and electrolytic cells in terms of the sign of ∆G.
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How voltaic cells use a spontaneous reaction to release electrical energy.
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The physical makeup of a voltaic cell: arrangement and composition of half-cells, relative charges of electrodes, and purpose of a salt bridge.
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How the difference in reducing strength of the electrodes determines the direction of electron flow in a voltaic cell.
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The correspondence between a positive E_cell and a spontaneous cell reaction.
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The usefulness and significance of standard electrode potentials (Eº_half-cells).
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How Eº_half-cell values are combined to give Eº_cell.
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How the standard reference electrode is used to find an unknown Eº_half-cell.
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How an emf series is used to write spontaneous redox reactions.
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How the relative reactivity of a metal is determined by its reducing power and is related to the negative of its Eº_half-cell.
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How E_cell (the nonstandard cell potential) is related to ∆G (maximum work) and the charge (moles of electrons times the Faraday constant) flowing through the cell.
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The interrelationship of ∆Gº, Eº_cell, and K.
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How E_cell changes as the cell operates (as Q changes).
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