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Question 20.7: Determining the Direction of Spontaneity from Electrode Pote...

Determining the Direction of Spontaneity from Electrode Potentials

Consider the reaction

\mathrm{Zn}^{2+}(a q)+2 \mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Zn}(s)+2 \mathrm{Fe}^{3+}(a q)

Does the reaction go spontaneously in the direction indicated, under standard conditions?


Find the oxidizing agents in the equation; one is on the left side and the other on the right side. Locate these oxidizing agents in a table of electrode potentials. (The oxidizing agent is on the left side of the reduction half-reaction.) The stronger oxidizing agent is the one involved in the half-reaction with the more positive standard electrode potential.

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