Galvanic Cells - Measurement of Electrode Potential

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^Θ and equilibrium constant of the reaction.

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

`Sn(s) | Sn^(2+) (0.004 M) || H^(+) (0.020 M) | H_2 (g) ("1 bar") | Pt(s)`

(Given: `E_(Sn^(2+)"/"Sn)^0 = -0.14` V)

In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to:-

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

Account for the following:

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

In a galvanic cell, current flows ______

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

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^θ and equilibrium constant of the reaction.