Question

For the following reaction, identify the element that was oxidized, the element that was reduced, and the oxidizing agent. Give an explanation for each answer.
Zn + H2SO4 ZnSO4 + H2

Answer 1

Answer: Element Zn is being oxidized, Element hydrogen is being reduced and it the oxidizing agent.

Explanation:

Oxidation reaction is defined as the reaction in which an element looses its electrons. The oxidation state is increased in these type of reaction.The element undergoing these reactions are said to be oxidized.

Reduction reaction is the reaction in which an element accepts electrons. The oxidation state decreases in these type of reactions. The element undergoing these reactions are said to be reduced.

Oxidizing agents are defined as the agents which helps in the oxidation of other element and itself gets reduced.

Reducing agents are defined as the agents which helps in the reduction of other element and itself gets oxidized.

For the given reaction:

$Zn+H_2SO_4\rightarrow ZnSO_4+H_2$

Zinc is getting oxidized to $Zn^{2+}$

Hydrogen is getting reduced to $H_2$

Oxidation reaction: $Zn\rightarrow Zn^{2+}+2e^-$

Reduction reaction: $2H^++2e^-\rightarrow H_2$

Here, hydrogen is considered as the reducing agent.

Answer 2

Oxidation is the Loss of electron 
Reduction is the Addition of Electron
Zn + H2SO4  ------>  ZnSO4 + H2

Zn(+2)/Zn ----------------------)       Zn ----------->Zn(+2) + 2e-
H(+)/H2 ------------------------)        2H(+) + 2e -------------> H2
So ,
 
Zn is the reducing agent and H+ is the oxidation agent
Therefore,
Zn is oxidized and H+ is reduced