A galvanic cell at 298 K employs the half-reactions The silver half-cell contains 0.025 M

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

Problem

A galvanic cell at 298 K employs the half-reactions Ag++e−→Ag(s)Ag^{+} + e^- \rightarrow Ag(s) E°=+0.80 VE^{\text{°}} = +0.80\,\text{V} Ni2++2e−→Ni(s)Ni^{2+} + 2e^- \rightarrow Ni(s) E°=−0.25 VE^{\text{°}} = -0.25\,\text{V} The silver half-cell contains 0.025 M Ag+Ag^{+}. The nickel half-cell contains 1.5 M Ni2+Ni^{2+}. (1) Part 1: (a) Write the balanced overall cell reaction as it would proceed spontaneously under standard conditions. (2) Part 2: (b) Calculate the cell potential at 298 K for the given ion concentrations. Show all steps leading to your numerical answer. (3) 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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