Galvanic Cells - Measurement of Electrode Potential

How would you determine the standard electrode potential of the system \[\ce{Mg^{2+} | Mg}\]?

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place:

\[\ce{Fe{^{2+}_{(aq)}} + Ag{^{+}_{(aq)}} -> Fe{^{3+}_{(aq)}} + Ag_{(s)}}\]

Calculate the Δ_rG° and equilibrium constant of the reaction.

Galvanization is applying a coating of ______.

Write the cell reaction and calculate the e.m.f of the following cell at 298 K:

Sn_(s) | Sn²⁺ (0.004 M) || H⁺ (0.020 M) | H_2(g) (1 bar) | Pt_(s)

(Given: `E_(Sn^(2+)"/"Sn)^° = -0.14` V)

What is the standard free energy change for the following reaction at room temperature? Is the reaction spontaneous?

\[\ce{Sn(s) + 2Cu^{2+}(aq) -> Sn^{2+}(aq) + 2Cu+(s)}\]

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place:

\[\ce{2Cr_{(s)} + 3Cd{^{2+}_{(aq)}} -> 2Cr{^{3+}_{(aq)}} + 3Cd}\]

Calculate the Δ_rG° and equilibrium constant of the reaction.

Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.

Account for the following:

E° value for the Mn³⁺/Mn²⁺ couple is highly positive (+1.57 V) as compare to Cr³⁺/Cr²⁺.