8. \( 0.1 \mathrm{M} \) potassium iodide \( +0.1 \mathrm{M} \) potassium ferricyanide \( E^{\circ}= \) oxidation half reaction \( E^{0}= \) reduction half reaction \( E^{o}= \) NIE Expected observations Experimental observations
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First, we need to write the balanced half-reactions for both the oxidation and reduction processes. Oxidation half-reaction (potassium iodide): 2Iā» ā Iā + 2eā» EĀ°(oxidation) = -0.54 V (you can find this value in a standard reduction potential table) Reduction Show moreā¦
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Ronald P.
Potassium iodide in solution reacts readily with many reagents. In the following reactions, identify the atoms that are being oxidized and reduced, and specify the oxidizing and reducing agents. $$ \begin{array}{l}{\text { a. } \mathrm{Cl}_{2}(g)+\mathrm{KI}(a q) \rightarrow \mathrm{KCl}(a q)+\mathrm{I}_{2}(s)} \\ {\text { b. } 2 \mathrm{FeCl}_{3}(a q)+2 \mathrm{KI}(a q) \rightarrow} \\ {\qquad 2 \mathrm{FeCl}_{2}(a q)+2 \mathrm{KCl}(a q)+\mathrm{I}_{2}(s)}\end{array} $$ $$ 2 \mathrm{CuCl}_{2}(a q)+4 \mathrm{KI}(a q) \rightarrow $$
OxidationāReduction Reactions and Electrochemistry
OxidationāReduction Reactions Between Nonmetals
Balance each redox reaction using the half-reaction method. (a) $\mathrm{K}(s)+\mathrm{Cr}^{3+}(a q) \longrightarrow \mathrm{Cr}(s)+\mathrm{K}^{+}(a q)$ (b) $\operatorname{Mg}(s)+\operatorname{Ag}^{+}(a q) \longrightarrow \operatorname{Mg}^{2+}(a q)+\operatorname{Ag}(s)$ (c) $\mathrm{Al}(s)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{A}^{3+}(a q)+\mathrm{Fe}(s)$
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