A galvanic cell is constructed by immersing a zinc electrode in a 1.0 M Zn solution…

CHEMISTRY · Multi-part · A Level · Chemistry · Electrode potentials · Electrode potentials

Problem

A galvanic cell is constructed by immersing a zinc electrode in a 1.0 M Zn

^{2+}

solution and a silver electrode in a 1.0 M Ag

^{+}

solution. The two half-cells are connected through a salt bridge, and an external wire joins the electrodes. Selected standard reduction potentials are reproduced below. Zn

^{2+}

+ 2 e

^{-}

\;\longrightarrow\;

Zn(s)

E^{\circ} = -0.76\;\text{V}

^{+}

+ e

^{-}

\;\longrightarrow\;

Ag(s)

E^{\circ} = +0.80\;\text{V}

(a) Write the balanced overall reaction that occurs when the cell operates spontaneously at standard conditions. (b) Calculate the standard cell potential

E^{\circ}_{\text{cell}}

for the reaction you wrote in part (a). (c) State whether the reaction is thermodynamically favored under standard conditions and justify your answer using the value calculated in part (b).

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