Consider a cell constructed at using the following half-cells: • | ( ) • ( ) |…

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

Problem

Consider a cell constructed at

25\,^{\circ}\text{C}

using the following half-cells: •

Mg(s)

Mg^{2+}

(

1.0\,\text{M}

) •

Ag^{+}

(

1.0\,\text{M}

) |

Ag(s)

Selected standard reduction potentials are provided below:

Mg^{2+} + 2\,e^{-} \rightarrow Mg(s)

E^{\circ} = -2.37\,\text{V}

Ag^{+} + e^{-} \rightarrow Ag(s)

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

Answer the questions that follow. (1) Part 1: Calculate the standard cell potential,

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

, for the spontaneous reaction that occurs when the two half-cells are connected. (2) Part 2: Based on your calculation, determine which metal serves as the anode and which serves as the cathode. (3) Part 3: Write the balanced overall net-ionic equation for the spontaneous reaction occurring in the cell. (4) Part 4: State the direction of electron flow in the external circuit, using the metal names in your answer.

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