1 Consider the following two cells Pt U4 0200 M UO22 0150 M

1) Consider the following two cells:

Pt | U⁴⁺ (0.200 M), UO₂²⁺ (0.150 M), H⁺ (0.300 M) | | Fe²⁺ (0.0100 M), Fe³⁺ (0.0250 M) | Pt

Pt | TiO²⁺ (0.790 M), Ti³⁺ (0.00918 M), H⁺ (0.0147 M) | | VO²⁺ (0.1340 M), V³⁺ (0.0784M), H⁺ (0.0538 M) | Pt

a) Calculate the potential of the two cells.

b) Write the overall balanced redox equations for the reactions above.

c) Calculate ?G for the conditions given for reactions above.

d) Calculate K for the conditions given for reactions above.

I don\'t want the answers, just the methods I should take to solve the problem. Thanks.

Solution

The first step is to determine the cell reaction and total cell potential.

In order for the cell to be galvanic, E⁰_cell > 0.

**Review Galvanic Cell Example Problem for the method to find cell potential of a galvanic cell.

For this reaction to be galvanic, the cadmium reaction must be the oxidation reaction. Cd ? Cd²⁺+ 2 e^- E⁰ = +0.403 V
Pb²⁺ + 2 e^- ? Pb E⁰ = -0.126 V

Pb²⁺(aq) + Cd(s) ? Cd²⁺(aq) + Pb(s)

and E⁰_cell = 0.403 V + -0.126 V = 0.277 V

The Nernst equation is:

E_cell = E⁰_cell - (RT/nF) x lnQ

where
E_cell is the cell potential
E⁰_cell refers to standard cell potential
R is the gas constant (8.3145 J/mol