Question

Consider these generic half-reactions. Half-reaction E° (V) X+(aq)+e−⟶X(s) 1.52 Y2+(aq)+2e−⟶Y(s) −1.17 Z3+(aq)+3e−⟶Z(s) 0.84 Identify the strongest oxidizing agent. X+ Y2+ X Z Y Z3+ Identify the weakest oxidizing agent. X Z3+ Y Y2+ Z X+ Identify the strongest reducing agent. Z3+ X+ Y2+ Z X Y Identify the weakest reducing agent. Y Z X+ X Y2+ Z3+ Which substances can oxidize Z ?

Answer 1

Answer:

     strongest oxidizing agent: $X^{+}$

     weakest oxidizing agent: $Y^{2+}$

     strongest reducing agent: Y

     weakest reducing agent: X

     $X^{+}$ 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:

                       $E_{X^{+}\mid X}^{0}(1.52V)> E_{Z^{3+}\mid Z}^{0}(0.84V)> E_{Y^{2+}\mid Y}^{0}(-1.17V)$

So, strongest oxidizing agent: $X^{+}$

     weakest oxidizing agent: $Y^{2+}$

     strongest reducing agent: Y

     weakest reducing agent: X

As reduction potential of the half cell $X^{+}\mid X$ is higher than the reduction potential of the half cell $Z^{3+}\mid Z$ therefore $X^{+}$ will oxidize Z into $Z^{3+}$ and itself gets converted into X.