Consult the table of standard electrode potential and suggest three substances that can oxidize `Fe^(2+)` ions under suitable conditions.
Text Solution
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Only those species can oxidise ferrous ions `(Fe^(2+))` whose standard reduction potential is more positive than `0.77V`. Thus, suitable oxidising agents will be `F_(2),Cl_(2),Br_(2)`.
The positive value of the standard electrode potential of Cu^(2+)//Cu indicates that.......
On the basis of standard electrode potential values, suggest which of the following reactions would take place? (Consult the book for E^(ϴ) value) (a) Cu+Zn^(2+)toCu^(2+)+Zn (b) Mg+Fe^(2+)toMg^(2+)+Fe (c ) Br_(2)+2Cl^(-)toCl_(2)+2Br^(-) (d) Fe+Cd^(2)toCd+Fe^(2+)
Calculating the emf from standard potentials: A galvanic cell consists of an Al electrode in a 1.0M Al(NO_(3))_(3) solution and an Fe electrode in a 1.0M Fe(NO_(3))_(2) solution. Calculate the standard emf of this electrohemical cell at 25^(@)C . Also write the cell reaction. Strategy: From the table of standard electrode potentials, write the two reduction half reaction and standard electrode potentials for the cell. Change the direction of the half-cell reaction corresponding tol the smaller (or more negative) electrode potential. Multiply the when the half-reactions are added the electrons cancel. The sum of the half-reactions is the cell reaction. Add the electrode potentials to get the cell emf.
