Electrochemistry
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Electrolytic/galvanic/voltaic cell is for
Converts chemical energy of spontaneous redox rn into electrical energy.
Salt bridge
Connects two solutions without mixing them and maintaining electrical neutrality
EMF
P.d between 2 electrodes of a cell when no current is drawn from it
Electrode potential
Pd between electrode & electrolyte Or The potential of electrode when it shows a tendency to undergo oxidation or reduction in its salt sol
Standard electrode potential
Electrode potential when conc. of all species is unity
Cell potential
Pd between 2 electrodes of a galvanic cell
E(cell) =
E(cath) - E(ano) Same for standard E(cell)
When is reduced form of standard E.P more stable than hydrogen gas?
When it is > 0
Which has max and min tendency to get reduced?
Flourine & Lithium
Fluorine is a strong ___ and weak ___
Oxidizing agent & weak reducing agent
E(Metal(n+)/M) =
E°(M(n+)/M) - 2.303RT/nF log[M]/[Mn+]
1 Faraday is
96500C
If E° is -ve
It is a stronger reducing agent
Oxidation potential
Potential of a electrode when it loses e’
Which element will get reduced easily
Element with greater oxidation potential
Which will act as cathode or anode?
One with higher reduction potential will be cathode
Movement of e’s is from
Anode to cathode
E°(cell) in terms of K(c) is
E°(cell) = 0.0591/n logK(c)
Work done by a cell
W = EMF × nF
Electrical work done by the system is
Spontaneous
ΔG =
-nFE(cell)
When is a rn spontaneous?
ΔG < 0 and E°(cell) > 0
ΔG° =
-2.303RT logK(c)
EMF of Cu
0.34V