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# Redox Reactions Calculator

Calculate the electrode potential for a half-reaction, with inputs being the concentrations and stoichiometric coefficients of the reactants and products, and the number of electrons transferred:

### Input Values:

 Standard Reduction Potentials (volts) = F2 (g) + 2 e- --> 2 F -) (aq) H2(g) + O2(g) + H3O+ (aq) +2 e(-) --> 4 H2O (l) PbO2 (s) + SO4(2-) (aq) +4 H3O+ (aq) + 2 e(-) --> PbSO4 (s) + 6 H2O (l) MnO4(-) (aq) + 8 H3O(+) (aq) + 5 e(-) --> Mn2(+) (aq) + 12 H2O (l) Au(3+) (aq) + 3 e(-) --> Au (s) Cl2 (g) + 2 e(-) --> 2 Cl(-) (aq) Cr2O7(2-) (aq) + 14 H3O(+) (aq) + 6 e(-) --> 2 Cr(3+) (aq) + 21 H2O (l) O2 (g) + 4 H3O(+) (aq) + 4 e(-) --> 6 H2O (l) Br2 (l) + 2 e(-) --> 2 Br(-) (aq) NO3(-) (qa) 4 H3O(+) (aq) + 3e(-) --> NO (g) + 6 (H2O (l) OCl(-) + H2O (l)+ 2 e(-) --> Cl(-) (aq) + 2 OH(-) (aq) Hg(2+) + 2 e(-) --> Hg (l) Ag(+) (aq)+ e(-) --> Ag (s) Hg2(2+)+ 2 e(-) --> Hg (l) I2 (s) + 2 e(-) --> 2 I(-) (aq) O2 (g) + 2 H2O (l)+ 4 e(-) --> 4 OH(-) Cu(2+) + 2 e(-) --> Cu (s) Sn(4+) (aq) + 2 e(-) --> Sn(2+) (aq) 2 H3O(+) (aq)+ 2 e(-) --> H2 (g) + 2 H2O (l) Sn(2+) (aq) + 2 e(-) --> Sn (s) Ni(2+) (aq) + 2 e(-) --> Ni (s) V(3+) (aq)+ 3 e(-) --> V(2+) (aq) PbSO4 (s) + 2 e(-) --> Pb (s) + SO4(2-) (aq) Cd(2+)(aq) + 2 e(-) --> Cd (s) Fe(2+)+ 2 e(-) --> Fe (s) Zn(2+) (aq) + 2 e(-) --> Zn (s) 2 H2O (l) + 2 e(-) --> H2 (g) + 2 OH(-) (aq) Al(3+) (aq) + 3 e(-) --> Al (s) Mg(2+) (aq) + 2 e(-) --> Mg (s) Na(+) (aq) + e(-) --> Na (s) K(+) (aq) + e(-) --> K (s) Li(+) + e(-) --> Li (s)

 Concentration of Reactant A (molar)= M Stoichiometric Coefficient of Reactant A= Concentration of Reactant B (molar)= M Stoichiometric Coefficient of Reactant B= Concentration of Product C (molar)= M Stoichiometric Coefficient of Product C= Concentration of Product D (molar)= M Stoichiometric Coefficient of Product D= Number of electrons transferred (n)=

### Results:

 Standard Potential E0(from table) = volts E (calculated)= volts

### Input Values:

 Potential of first half-reaction (be careful with sign!)= Potential of second half-reaction (be careful with sign!)=

### Results:

 E (calculated)= volts

Developed by
Shodor
in cooperation with the Department of Chemistry,
The University of North Carolina at Chapel Hill