A galvanic cell is constructed using a copper electrode immersed in 1.0 L of a CuSO…

CHEMISTRY · Multi-part · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry

Problem

A galvanic cell is constructed using a copper electrode immersed in 1.0 L of a CuSO

_4

solution and a zinc electrode immersed in 1.0 L of a ZnSO

_4

solution. The temperature is 298 K. Initially, the Cu

^{2+}

concentration is 0.010 M and the Zn

^{2+}

concentration is 1.0 M. Standard reduction potentials (25 °C): Cu

^{2+}

+ 2 e

^-

→ Cu(s)

E^{\rm o} = +0.34\,\text{V}

^{2+}

+ 2 e

^-

→ Zn(s)

E^{\rm o} = -0.76\,\text{V}

(1) Part 1: (a) Identify the species that is reduced and the direction of electron flow through the external circuit for the initial conditions. (2) Part 2: (b) Without performing a numerical calculation, compare the initial cell potential to the standard cell potential. Clearly explain the reasoning that leads to your qualitative prediction. (3) Part 3: (c) Describe qualitatively how the magnitude of the cell potential will change as the cell operates and the concentrations of Cu

^{2+}

and Zn

^{2+}

approach their equilibrium values. Include an explanation that connects the change in potential to the position of equilibrium.

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