identify the reducing agent and oxidizing agent after writing out the following reaction: permanganate ion +…
identify the reducing agent and oxidizing agent after writing out the following reaction: permanganate ion + sulfur dioxide producing sulfate ion + manganese(ii) ion\nreducing agent: sulfur dioxide oxidizing agent: manganese(ii) ion\nreducing agent: manganese(ii) ion oxidizing agent: sulfate ion\nreducing agent: sulfate ion oxidizing agent: sulfur dioxide\nreducing agent: manganese(ii) ion oxidizing agent: sulfur dioxide\nreducing agent: sulfur dioxide oxidizing agent: permanganate ion\nreducing agent: sulfur dioxide oxidizing agent: sulfate ion\nreducing agent: sulfate ion oxidizing agent: permanganate ion\nreducing agent: permanganate ion oxidizing agent: manganese(ii) ion\nreducing agent: permanganate ion oxidizing agent: sulfate ion\nreducing agent: permanganate ion oxidizing agent: sulfur dioxide
Answer
Explanation:
Step1: Write the half - reactions
Oxidation half - reaction: $SO_{2}+2H_{2}O\rightarrow SO_{4}^{2 - } + 4H^{+}+2e^{-}$. Sulfur in $SO_{2}$ has an oxidation state of +4 and in $SO_{4}^{2 - }$ it is +6. So, $SO_{2}$ is oxidized. Reduction half - reaction: $MnO_{4}^{-}+8H^{+}+5e^{-}\rightarrow Mn^{2 + }+4H_{2}O$. Manganese in $MnO_{4}^{-}$ has an oxidation state of +7 and in $Mn^{2 + }$ it is +2. So, $MnO_{4}^{-}$ is reduced.
Step2: Identify the agents
A reducing agent is a substance that is oxidized and donates electrons. Here, sulfur dioxide ($SO_{2}$) is the reducing agent. An oxidizing agent is a substance that is reduced and accepts electrons. Here, permanganate ion ($MnO_{4}^{-}$) is the oxidizing agent.
Answer:
reducing agent: sulfur dioxide, oxidizing agent: permanganate ion