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

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

Here's why:

1. Identify the oxidation states of each element in the reaction. The oxidation state of Pb in Pb(s) is 0. The oxidation state of Ag in AgNO3 is +1. In the products, the oxidation state of Pb in Pb(NO3)2 is +2 and the oxidation state of Ag in Ag(s) is 0.

2. Determine the changes in oxidation states. Pb goes from an oxidation state of 0 to +2, which means it is oxidized (loses electrons). Ag goes from an oxidation state of +1 to 0, which means it is reduced (gains electrons).

3. Identify the oxidizing and reducing agents. The oxidizing agent is the substance that is reduced (gains electrons), so AgNO3 is the oxidizing agent. The reducing agent is the substance that is oxidized (loses electrons), so Pb is the reducing agent.