Respuesta :
Answer:
strongest oxidizing agent: [tex]X^{+}[/tex]
weakest oxidizing agent: [tex]Y^{2+}[/tex]
strongest reducing agent: Y
weakest reducing agent: X
[tex]X^{+}[/tex] will oxidize Z
Explanation:
The higher the reduction potential of a species, higher will be the tendency to consume electrons from another species. Hence higher will be the oxidizing power of it's oxidized form and lower will be the reducing power of it's reduced form.
Alternatively, higher reduction potential value suggests that the oxidized form of the species acts as a stronger oxidizing agent and the reduced form of the species acts as a weaker reducing agent.
Order of reduction potential:
[tex]E_{X^{+}\mid X}^{0}(1.52V)> E_{Z^{3+}\mid Z}^{0}(0.84V)> E_{Y^{2+}\mid Y}^{0}(-1.17V)[/tex]
So, strongest oxidizing agent: [tex]X^{+}[/tex]
weakest oxidizing agent: [tex]Y^{2+}[/tex]
strongest reducing agent: Y
weakest reducing agent: X
As reduction potential of the half cell [tex]X^{+}\mid X[/tex] is higher than the reduction potential of the half cell [tex]Z^{3+}\mid Z[/tex] therefore [tex]X^{+}[/tex] will oxidize Z into [tex]Z^{3+}[/tex] and itself gets converted into X.
The strongest reducing agent Y2+ and the weakest reducing agent is X+.
The more positive the reduction potential of a specie is, the better it serves as an oxidizing agent and is better able to accept electrons. In a nutshell, the specie that has a higher positive reduction potential is a better oxidizing agent. The reducing agent is the specie that has the most negative reduction potential.
Looking the half reaction equations;
- X+(aq)+e−⟶X(s) 1.52 V
- Y2+(aq)+2e−⟶Y(s) −1.17 V
- Z3+(aq)+3e−⟶Z(s) 0.84 V
We can see that the strongest oxidizing agent is X+, the weakest oxidizing agent is Y2+, the strongest reducing agent Y2+ and the weakest reducing agent is X+.
Learn more: https://brainly.com/question/14191541
