Chemistry

Problem

A galvanic cell at 298 K employs the half-reactions

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

E^{\text{°}} = +0.80\,\text{V}

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

E^{\text{°}} = -0.25\,\text{V}

The silver half-cell contains 0.025 M

Ag^{+}

. The nickel half-cell contains 1.5 M

Ni^{2+}

. a. Part 1: (a) Write the balanced overall cell reaction as it would proceed spontaneously under standard conditions. b. Part 2: (b) Calculate the cell potential at 298 K for the given ion concentrations. Show all steps leading to your numerical answer. c. Part 3: (c) State whether the reaction is spontaneous in the direction written in part (a) under the given non-standard conditions. Justify your answer by referencing the sign of the calculated potential.

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