1. Which of the following reactions are spontaneous at standard state? (Consult table of electrode potentials.)
A) $\mathrm{I}_{2}+2 \mathrm{Fe}^{2+} 3 / 4 ® 2 \mathrm{I}^{-}+2 \mathrm{Fe}^{3+}$
B) $8 \mathrm{H}^{+}+2 \mathrm{NO}_{3}^{-+}+3 \mathrm{Cu}_{(\mathrm{s})} 3 / 4 \mathbb{R}_{2} \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{Cu}^{2+}+4 \mathrm{H}_{2} \mathrm{O}$
C) $4 \mathrm{MnO}_{4}^{-+}+12 \mathrm{H}^{+} 3 / 4 \mathrm{R}_{4} \mathrm{Mn}^{2+}+5 \mathrm{O}_{2}+6 \mathrm{H}_{2} \mathrm{O}$
D) $\mathrm{Cu}_{(\mathrm{s})}+\mathrm{Cl}_{2(\mathrm{~g})} 3 / 4 ® \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Cl}_{(\mathrm{aq})}$

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***D*** ∻Key Concept∻ ⚹Spontaneity and Electrode Potentials⚹ ∻Explanation∻ ⚹A spontaneous reaction at standard state occurs when the overall cell potential is positive. This is determined by looking up the standard electrode potentials for the half-reactions and calculating the standard cell potential (E°cell). If E°cell is positive, the reaction is spontaneous.⚹◊What is the standard electrode potential for the reaction presented in option C⍭ Generate me a similar question◊

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