Question

consider the reaction
2MnO4+5CO2O4²+16H(aq)

Answer 1

2MnO4 is the oxidizing agent. Cl is the reducing agent. 16H IS NOT A REDUCING AGENT. It took me a while to figure this out because in your reactants, it should say 10Cl ^ -. An atom of chlorine has a charge of negative one.

Answer 2

Answer:

Redox reactions are those chemical processes in which both oxidation and reduction take place at the same time. The material that initiates the oxidation of any other substance during a reaction is referred to as the oxidizing agent, while the substance that initiates the reduction is referred to as the reducing agent.

Explanation:

In the given redox reaction that occurs in the presence of acidic medium results in,

• the oxidation state of manganese changes from +7 to +2. The oxidation state decreases and this results from the reduction of $MnO_{4}^{-}$ to $Mn^{2+}$.

• the oxidation state of carbon changes from +3  to +4. The oxidation state increases and this results from the oxidation of $C _{2} O_{4}^{2-}$ to $CO_{2}$.

Thus, $MnO_{4}^{-}$ acts as an oxidizing agent and $C_{2} O_{4}^{2-}$ acts as a reducing agent.

Hence, the complete redox reaction is $2 MnO_{4}^{-} + 5 C_{2} O_{4}^{2-} + 16 H^{+}$ →$2 Mn^{2+} + 10 CO_{2} + 8 H_{2} O$ .

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