Final answer:
In the reaction 2Cl₂ + Sn → SnCl₄, tin (Sn) acts as the reducing agent by being oxidized, and chlorine (Cl₂) acts as the oxidizing agent by being reduced.
Step-by-step explanation:
To identify the reducing agent and oxidizing agent in the chemical reaction 2Cl₂ + Sn → SnCl₄, we need to look at the changes in oxidation states of the reactants and products. The tin (Sn) starts with an oxidation state of 0 and ends up with an oxidation state of +4 in the stannic chloride (SnCl₄), which means it loses electrons and is being oxidized, thus Sn is the reducing agent. On the other hand, each chlorine (Cl₂) molecule starts with an oxidation state of 0 and ends up with an oxidation state of -1 in SnCl₄, which means chlorine gains electrons and is being reduced; hence, Cl₂ is the oxidizing agent.