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Nernst equation halps us to understand t...

Nernst equation halps us to understand the effect of `"______"` on the electrode of the half-cell and `emf` of the voltiv cell

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Calculating the cell emf for Nonstandard condition : A galvanic cell is constructed at 298 K as follows. One half-cell consists of a chlorine gas electrode (i.e. Cl_(2)//Cl^(-) couple) with the partial pressure of Cl_(2) = 0.100 bar and C_(CI-) = 0.100 M . The other half-cell involves the MnO_(4)^(-)//Mn^(2+) couple in acidic solution with C_(MnO_(4)^(-)) = 0.100 M, C_(Mn^(2+)) = 0.100 M , and C_(H+) = 1.00 M . Apply the Nernst equation to datermine the cell potenital for this cell. Strategy: First datermine the overall cell reaction and then calculate the standard cell potential (E_("cell")^(@)) from the standard electrode potenital in Table 3.1. then use the Nernst equation to find the cell potential (E) under cited conditions.

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.