Previous Tries were:
1st Try:
2H2O --> O2 + 4H+ + 4e-
Ag --> Ag+ + e-
2F- --> F2 + 2e-
F2 + 2e- --> 2F-
Second Try:
O2 + 4H+ + 4e- --> 2H2O
Ag --> Ag+ + e-
2H2O --> O2 + 4H+ + 4e-
F2 + 2e- --> 2F-
During the electrolysis ,
reduction takesplace at cathode and oxidtion at anode.
1) electrolysis of 0.100 aqueous KF
here both water and KF are present
As the discharge potential of H+ to H2 is less than that of K+ , at cathode H2 is liberated NOT K.
So reduction of H2O at cathode.
2H2O +2e- ------------> H2 + 2OH-
Q2)
1.0M AgNO3
At anode H2O is oxidised O2 as NO3- has very high reduction potential than H2O.
The reaction is
2H2O -----> O2 + 4H+ + 4 e-
Q3)
At anode oxidation of water (or OH-) to O2 takesplace as F- has higher potential than OH-.
Thus oxidation at anode is
2H2O -----> O2 + 4H+ + 4 e-
Q4)with molten KF
at cathode the only cation is K+ that can be reduced.
So the reduction half reaction at cathode is
K+ + e- -----> K
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