Question

Which species functions as the oxidizing agent in the following reduction-oxidation reaction:
Zn(s) + Cu^2+(aq) ---> Cu(s) + Zn^2+(aq)
A) Zn^2+(aq)
B) Zn(s)
C) Cu^2+
D) Cu(s)

Answer 1

Answer: $Cu^{2+}(aq.)$ is the oxidizing agent for the given equation.

Explanation:

Reduction reaction is defined as the reaction in which a substance gains electrons.

Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions.

Oxidation reaction is defined as the reaction in which a substance looses its electrons.

Reducing agents are defined as the agents which reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.

For the given chemical equation:

$Zn(s)+Cu^{2+}(aq.)\rightarrow Cu(s)+Zn^{2+}(aq.)$

The half reaction follows:

Oxidation half reaction:  $Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-$

Reduction half reaction:  $Cu^{2+}(aq.)+2e^-\rightarrow Cu(s)$

As, zinc is getting oxidized, it is considered as a reducing agent and copper is getting reduced, it is considered as an oxidizing agent.

Hence, $Cu^{2+}(aq.)$ is the oxidizing agent for the given equation.