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In the following chemical reaction, which substance is the oxidizing agent and which is the reducing agent?Mn(s)  +  2 AgNO3(aq)  →  Mn(NO3)2(aq)  +  2 Ag(s)oxidizing agent: reducing agent:

Question

In the following chemical reaction, which substance is the oxidizing agent and which is the reducing agent?Mn(s)  +  2 AgNO3(aq)  →  Mn(NO3)2(aq)  +  2 Ag(s)oxidizing agent: reducing agent:

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Solution

In this chemical reaction, the oxidizing agent is AgNO3 and the reducing agent is Mn.

Here's why:

  1. Identify the oxidation states of each element in the reaction. In Mn(s), Mn is in its elemental state, so its oxidation state is 0. In AgNO3, Ag is in +1 oxidation state. In Mn(NO3)2, Mn is in +2 oxidation state. In Ag(s), Ag is in its elemental state, so its oxidation state is 0.

  2. Determine which elements have changed oxidation state. Mn has gone from an oxidation state of 0 to +2, meaning it has been oxidized (lost electrons). Ag has gone from an oxidation state of +1 to 0, meaning it has been reduced (gained electrons).

  3. The substance that is oxidized is the reducing agent, and the substance that is reduced is the oxidizing agent. Therefore, Mn is the reducing agent and AgNO3 is the oxidizing agent.

This problem has been solved

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