Cell E and Cell F are based on the reaction with

CHEMISTRY · Single correct · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry

Problem

Cell E and Cell F are based on the reaction

\mathrm{2Ag^{+}(aq)+Fe(s)\rightarrow 2Ag(s)+Fe^{2+}(aq)}

with

E^{\circ}=1.24\,\text{V}

. Cell E:

[\mathrm{Ag^{+}}]=0.010\,\text{M}

and

[\mathrm{Fe^{2+}}]=1.0\,\text{M}

Cell F:

[\mathrm{Ag^{+}}]=1.0\,\text{M}

and

[\mathrm{Fe^{2+}}]=0.010\,\text{M}

298\,\text{K}

, which statement correctly identifies which cell’s instantaneous potential deviates more from

E^{\circ}

and provides the primary reason? (a) Both cells deviate equally because the squared silver concentration balances the opposite concentration changes. (b) Cell E deviates more because its larger reaction quotient produces a greater opposing term in the Nernst equation. (c) Cell F deviates more because its reactant-favored (Q<1) conditions raise the cell potential above

E^{\circ}

by a larger amount. (d) The deviation cannot be compared since the presence of solids prevents an exact value for the reaction quotient.

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