Increase in oxidation number is known as oxidation and decrease in oxidation number is known as reduction.
Oxidation half reaction :-
Fe ----> Fe^3+ + 3e^- -------(1)
Reduction half reaction :-
ClO4^- + 8H^+ + 8e^- ------> Cl^- + 4H2O -------(2)
Multiply (1) by 8 and (2) by 3 and then add it
8Fe -----> 8Fe^3+ + 24 e^-
3ClO4^- + 24 H^+ + 24 e^- -----> 3Cl^- + 12 H2O
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8Fe + 3ClO4^- + 24 H^+ ------> 8Fe^3+ + 3Cl^- + 12 H2O
Balance the following electrochemical equation for an acidic environment. C104" + Fe → C1- + Fe3+
Balance the following electrochemical equation for an acidic
environment.
C104" + Fe → C1- + Fe3+
Balance the following electrochemical equation for an acidic
environment.
C104" + Fe → C1- + Fe3+
2) Balance the following electrochemical equation for a basic environment. Cr + Cut → Cu + C104
1) Balance the following electrochemical equation for an acidic environment. Cro42 + Zn → Zn2+ + Cr+
2) Balance the following electrochemical equation for a basic environment. CT + Cut → Cu + C104
1) Balance the following electrochemical equation for an acidic environment. CrO4+Zn Zn2 +Cr
Balance the following electrochemical equation for an acidic environment. H_2CrO_4 + Ti rightarrow Cr^3+ + Ti^4+
Balance the following reactions (acidic solution). Cr2O72- + Cl + Cr2+ + HCIO H3PO4 + Fe → PH3 + Fe3+ I' + C104 → 13' +Cl-
Balance the following electrochemical equation for a basic
environment.
NH3 + Cu2+ NO + Cu
2) Balance the following electrochemical equation for a basic environment. CI" + Cut → Cu + CIO4