Question

This one is a bit long but I am desperate!

Use the equation below to answer the following questions.
Ba + ZnSO4 BaSO4 + Zn

a. Determine the oxidation state of the atoms in the equation reactants and products:

Oxidation state of Ba in reactant:
In product:

Oxidation state of Zn in reactant:
In product:

Oxidation state of S in reactant:
In product:

Oxidation state of O in reactant:
In product:

Explain why this is a redox reaction.

b. Write the half-reactions for the reaction. Label the oxidation reaction and the reduction reaction.


c. In this equation, what was oxidized and what was reduced?

d. In this equation, what is the oxidizing agent and what is the reducing agent?

Answer 1

a) Oxidation state of Ba in reactant: 0
In product: +2.
Oxidation state of Zn in reactant: +2.
In product: 0.
Oxidation state of S in reactant: +6
In product: +6.
Oxidation state of O in reactant: -2.
In product: -2.
This is redox reaction because elements change their oxidation states (barium and zinc).
b) Oxidation reaction: Ba⁰ → Ba²⁺ + 2e⁻.
Reduction reaction: Zn²⁺ + 2e⁻ → Zn⁰.
c) Barium is oxidized (increase of oxidation number) and zinc is reduced (decrease of oxidation number).
d)  The oxidizing agent is zinc (gain electrons) and the reducing agent is barium (lose electrons).