1) Consider the following two cells: Pt | U 4+ (0.200 M), UO 2 2+ (0.150 M), H +

Question

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.

Explanation / Answer

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

In order for the cell to be galvanic, E0cell > 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 E0cell = 0.403 V + -0.126 V = 0.277 V

The Nernst equation is:

Ecell = E0cell - (RT/nF) x lnQ

where
Ecell is the cell potential
E0cell refers to standard cell potential
R is the gas constant (8.3145 J/mol

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