A galvanic cell is assembled at 298 K using the following half-reactions:…

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

Problem

A galvanic cell is assembled at 298 K using the following half-reactions: Mg2+(aq)+2e−→Mg(s)

E^{\rm o}=-2.37\,\text{V}

Cu2+(aq)+2e−→Cu(s)

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

The cell is arranged so that solid magnesium is the anode and solid copper is the cathode. At the moment of assembly the ion concentrations are [Mg2+]=0.010 M and [Cu2+]=1.00 M. (1) Part 1: (a) Write the balanced overall cell reaction, clearly indicating the direction of electron flow through the external circuit. (2) Part 2: (b) Determine the numerical value of the cell potential

E_{\text{cell}}

(in volts) under the stated non-standard conditions at 298 K. Show your work clearly and report your answer to the appropriate number of significant figures. (3) Part 3: (c) State whether the calculated cell potential is larger or smaller in magnitude than

E^{\rm o}_{\text{cell}}

for this system, and explain qualitatively why that is the case.

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