Calculate Equilibrium Constant for Spontaneous Cell Reaction | Electrochem Help

[geffman1]

Homework Statement

Refer to the cell below:
Pt / MnO4-(0.10 M), Mn2+(0.20 M).H+(0.010M) // Cr3+(0.40 M), Cr2O72-(0.30 M), H+(0.010M) / Pt
The standard reduction potentials are as follows:
MnO4- + 8H+ + 5e- --> Mn2+ + 4H2O; E° = 1.51 V
Cr2O72- + 14 H+ + 6e- --> 2 Cr3+ + 7H2O; E° = 1.33 V
What is the value of the equilibrium constant at 25°C for the net spontaneous cell reaction?



a. 7.3 x 10^-11

b. 6.1 x 10^-92

c. 91

d. 1.1 x 10^3

e. 2.1 x 10^91

any help would br greatful appreciated. thanks

 

[Borek]

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