Define Standard Hydrogen Electrode(SHE)
SHE consists of H2(g) @ 1 bar bubbling over platinised Pt electrode which is dipped into 1moldm-3 H+ solution @ 298K
Define Standard Cell Potential(Eocell)
electromotive force(emf) of galvanic cell which connects 2 half-cells under standard conditions. The Eocell value is the diff. b/w standard electrode potential(Eo) of 2 half-cells.
Eocell = Eocathode - Eoanode
Define Eo of half-cell
relative [R] potential of this half-cell under stc as compared w/ standard hydrogen electrode whose EO is assigned as 0.00V
(a) describe and explain redox processes in terms of electron transfer and/or of
changes in oxidation number (oxidation state)
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(b) define the terms:
(i) standard electrode (redox) potential
(ii) standard cell potential
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(c) describe the standard hydrogen electrode
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(d) describe the methods used to measure the standard electrode potentials of:
(i) metals or non–metals in contact with their ions in aqueous solution
(ii) ions of the same element in different oxidation states
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(e) calculate a standard cell potential by combining two standard electrode potential
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(f) use standard cell potentials to:
(i) explain/deduce the direction of electron flow from a simple cell
(ii) predict the spontaneity of a reaction
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(g) understand the limitations in the use of standard cell potentials to predict the spontaneity of a reaction
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(h) construct redox equation using the relevant half–equations
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(i) state and apply the relationship ∆GƟ = ∆nFEƟ to electrochemical cells, including the calculation of EƟ for combined half reactions
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(j) predict qualitatively how the value of an electrode potential varies with the
concentration of aqueous ion
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(k) state the possible advantages of developing other types of cell, e.g.s the H2/O2 fuel cell and improved batteries (as in electric vehicles) in terms of smaller size, lower mass and higher voltage.
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