What is the cell potential for the spontaneous concentration cell with the react

Question

What is the cell potential for the spontaneous concentration cell with the reaction Fe^3+(aq) + Fe(s) rightarrow Fe(s) + Fe^3+(aq), with concentrations of Fe^3+ of 0.811M and 0.379M at a temperature of 310. K? E_cell = E_cell^degree - (RT/nF)lnQ Which of the following will decrease the cell potential for the following reaction 2Fe^3+(aq) + 3Zn(s) rightarrow 3Zn^2+(aq) + 2Fe(s) Use the reaction E_cell = E_cell^degree - (RT/nF)lnQ and consider how each manipulation affects Q and thus affects E_cell Add zinc solid Remove water from the entire system Increase concentration of Fe^3+ in the solution Dilute the entire system Add solid iron to the system increase the concentration of zinc ion in solution

Explanation / Answer

1)

At 310 K,

RT/F = 8.314*310/96485 = 0.0267

Number of electron being transferred in balanced reaction is 3

So, n = 3

Use:

E = Eo - (RT/nF) ln {[Fe3+]/[Fe3+]}

E = 0 - (0.0267/n) ln {[Fe3+]/[Fe3+]}

E = - (0.0267/3) ln (0.379/0.811)

E = 6.77*10^-3 V

Answer: 6.77*10^-3 V

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