The table below lists standard electrode potentials measured at

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

Problem

298\,\text{K}

. Half-Reaction (all potentials vs. SHE) 1.

Cu^{2+}

(aq) + 2

e^{-}

→ Cu(s)

E^\circ = +0.34\,\text{V}

Zn^{2+}

(aq) + 2

e^{-}

→ Zn(s)

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

A galvanic cell is assembled by immersing a copper strip in

1.0\,\text{M}

Cu^{2+}

(aq) solution and a zinc strip in

1.0\,\text{M}

Zn^{2+}

(aq) solution. The two half-cells are connected by a salt bridge, and a high-resistance voltmeter is wired between the metal electrodes. (a) Write the balanced overall redox equation for the spontaneous reaction occurring in the cell, including physical states. (b) Calculate the standard cell potential,

E^\circ_{cell}

, for the reaction written in part (a). Show all work, including the numerical value with the correct sign and units. (c) Using the value obtained in part (b), determine the sign of

\Delta G^\circ

for the reaction and explain in words what this sign indicates about the spontaneity of the process under standard conditions.

Related theory

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