Question

In the following 2 questions, determine what is being oxidized and what is being reduced in each reaction. Identify the oxidizing and reducing agents in each :

a. 2Mg(s) + O2(g) → 2MgO(s)
b. Pb(NO3)2(aq) + Zn(s) → Zn(NO3)2(aq) +Pb(s)

Answer 1

a) Mg is oxidized and O2 is reduced

b) Zn is oxidized while Pb(NO3)2 is reduced.

Oxidation and reduction

Oxidation is defined as:

1. loss of electrons
2. removal of hydrogen
3. addition of oxygen
4. increase in oxidation number
5. removal of electropositive elements

Reduction is defined as:

1. gains of electrons
2. addition of hydrogen
3. removal of oxygen
4. decrease in oxidation number
5. addition of electropositive elements

Looking at the first reaction, the Mg atom gains oxygen to become MgO. This means that Mg is oxidized. The oxidizing agent is O2. At the same time, O2 is being reduced and the reducing agent is Mg.

For the second reaction, the oxidation number of Pb is reduced from +2 to 0. Thus, Pb has been reduced by Zn while Zn itself has been oxidized. The reducing agent here is Zn while the oxidizing agent is Pb(NO3)2.

More on oxidation and reduction can be found here: https://brainly.com/question/13699873

#SPJ1