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CHEM 113- Unit 5

ΔG when K is small positive (non-spontaneous)
ΔG when K is large negative (spontaneous)
redox reactions- acid solutions balance O with H2O, balance H with H+
redox reactions- basic solutions remove H+ with OH-, reconcile H2O's
anode oxidation (metal breaks down, more ions added to solution)
cathode reduction (metal builds up, ions removed from solution)
salt bridge allow transfer of ions (anions toward anode; cations toward cathode)
inactive electrodes electrodes made of something different than the solutions but still transfer electrons
2 most common inactive electrodes carbon, poladium, platinum
voltaic cell notation inactive electrode|lower ox state|higher ox state||higher ox state|lower ox state|inactive electrode
Ecell= cathode-anode
Voltaic cells are spontaneous when Ecell>0
Reduction potential is based off of standard hydrogen electrode
metal activity higher reduction potential=higher activity
concentration cell same metal at the anode and cathode-> differ in concentration (anode is always lower)
electrolytic cell external source of power must be greater than Ecell for the forward reaction
sign of oxidation in an electrolytic cell +
sign of reduction in an electrolytic cell -
molten salts: what forms at the anode LESS electronegative non-metal
molten salts: what forms at the cathode MORE electronegative metal
Created by: melaniebeale