(j) MnO_(4)^-+Mn^2++OH^-arrow MnO_(2)(s) 0. Identify the oxidizing agent and the reducing agent on the left side of each equation in Problem 18-9; write a balanced equation for each half-reaction. 1. Consider the following oxidation/reduct ion reactions: AgBr(s)+V^2+arrow Ag(s)+V^3++Br^- TI^3++2Fe(CN)_(6)^4-arrow TI^++2Fe(CN)_(6)^3- 2V^3++Zn(s)arrow 2V^2++Zn^2+ Fe(CN)_(6)^3-+Ag(s)+Br^-arrow Fe(CN)_(6)^4-+AgBr(s) S_(2)O_(8)^2-+Tl^+arrow 2SO_(4)^2-+Tl^3+ (a) Write each net process in terms of two balanced (b) Express each half -reaction as a reduction. (-) A. __ the half. __ in (h)

Let's break down the problem step by step:<br /><br />### Part (j): Identifying the Oxidizing and Reducing Agents<br /><br />Given the reaction:<br />\[ MnO_{4}^{-} + Mn^{2+} + OH^{-} \rightarrow MnO_{2}(s) \]<br /><br />1. **Identify the Oxidizing Agent:**<br /> - The oxidizing agent is the species that gets reduced. In this case, \( MnO_{4}^{-} \) is reduced to \( MnO_{2} \).<br /> - The reduction half-reaction is:<br /> \[ MnO_{4}^{-} + 2H_{2}O + 3e^{-} \rightarrow MnO_{2} + 4OH^{-} \]<br /><br />2. **Identify the Reducing Agent:**<br /> - The reducing agent is the species that gets oxidized. In this case, \( Mn^{2+} \) is oxidized to \( MnO_{2} \).<br /> - The oxidation half-reaction is:<br /> \[ Mn^{2+} + 2H_{2}O \rightarrow MnO_{2} + 2H^{+} + 2e^{-} \]<br /><br />### Part 1: Balancing Half-Reactions<br /><br />Consider the following oxidation/reduction reactions:<br /><br />1. \( AgBr(s) + V^{2+} \rightarrow Ag(s) + V^{3+} + Br^{-} \)<br /><br /> - **Oxidation Half-Reaction:**<br /> \[ V^{2+} \rightarrow V^{3+} + e^{-} \]<br /><br /> - **Reduction Half-Reaction:**<br /> \[ AgBr(s) + e^{-} \rightarrow Ag(s) + Br^{-} \]<br /><br />2. \( TI^{3+} + 2Fe(CN)_{6}^{4-} \rightarrow TI^{+} + 2Fe(CN)_{6}^{3-} \)<br /><br /> - **Reduction Half-Reaction:**<br /> \[ TI^{3+} + e^{-} \rightarrow TI^{+} \]<br /><br /> - **Oxidation Half-Reaction:**<br /> \[ 2Fe(CN)_{6}^{4-} \rightarrow 2Fe(CN)_{6}^{3-} + e^{-} \]<br /><br />3. \( 2V^{3+} + Zn(s) \rightarrow 2V^{2+} + Zn^{2+} \)<br /><br /> - **Reduction Half-Reaction:**<br /> \[ 2V^{3+} + 2e^{-} \rightarrow 2V^{2+} \]<br /><br /> - **Oxidation Half-Reaction:**<br /> \[ Zn(s) \rightarrow Zn^{2+} + 2e^{-} \]<br /><br />4. \( Fe(CN)_{6}^{3-} + Ag(s) + Br^{-} \rightarrow Fe(CN)_{6}^{4-} + AgBr(s) \)<br /><br /> - **Reduction Half-Reaction:**<br /> \[ Fe(CN)_{6}^{3-} + e^{-} \rightarrow Fe(CN)_{6}^{4-} \]<br /><br /> - **Oxidation Half-Reaction:**<br /> \[ Ag(s) + Br^{-} \rightarrow AgBr(s) + e^{-} \]<br /><br />5. \( S_{2}O_{8}^{2-} + Tl^{+} \rightarrow 2SO_{4}^{2-} + Tl^{3+} \)<br /><br /> - **Reduction Half-Reaction:**<br /> \[ S_{2}O_{8}^{2-} + 2e^{-} \rightarrow 2SO_{4}^{2-} \]<br /><br /> - **Oxidation Half-Reaction:**<br /> \[ Tl^{+} \rightarrow Tl^{3+} + 3e^{-} \]<br /><br />### Part (a): Writing Net Processes in Terms of Two Balanced Half-Reactions<br /><br />For each net process, write it in terms of two balanced half-reactions:<br /><br />1. \( AgBr(s) + V^{2+} \rightarrow Ag(s) + V^{3+} + Br^{-} \)<br /><br /> - **Oxidation Half-Reaction:**<br /> \[ V^{2+} \rightarrow V^{3+} + e^{-} \]<br /><br /> - **Reduction Half-Reaction:**<br /> \[ AgBr(s) + e^{-} \rightarrow Ag(s) + Br^{-} \]<br /><br />2. \( TI^{3+} + 2Fe(CN)_{6}^{4-} \rightarrow TI^{+} + 2Fe(CN)_{6}^{3-} \)<br /><br /> - **Reduction Half-Reaction:**<br /> \[ TI^{3+} + e