Questions: Consider these generic half-reactions. Half-reaction E°(V) X+(aq) + e- -> X(s) 0.84 Y2+(aq) + 2 e- -> Y(s) -1.17 Z3+(aq) + 3 e- -> Z(s) 1.52 Identify the strongest oxidizing agent. X Y X+ Z Y2+ Z3+ Identify the strongest reducing agent. Z3+ Y Z Y2+ X+ x Identify the weakest oxidizing agent. X Y Z X+ Y2+ Z3+ Identify the weakest reducing agent. X Y X+ z3+ Y2+ Z

Consider these generic half-reactions.

Half-reaction E°(V)
X+(aq) + e- -> X(s) 0.84
Y2+(aq) + 2 e- -> Y(s) -1.17
Z3+(aq) + 3 e- -> Z(s) 1.52

Identify the strongest oxidizing agent.
X
Y
X+
Z
Y2+
Z3+

Identify the strongest reducing agent.
Z3+
Y
Z
Y2+
X+
x

Identify the weakest oxidizing agent.
X
Y
Z
X+
Y2+
Z3+

Identify the weakest reducing agent.
X
Y
X+
z3+
Y2+
Z

Transcript text: Consider these generic half-reactions. Half-reaction & $E^{\circ}(\mathrm{V})$ \\ $\mathrm{X}^{+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{X}(\mathrm{s})$ & 0.84 \\ $\mathrm{Y}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \longrightarrow \mathrm{Y}(\mathrm{s})$ & -1.17 \\ $\mathrm{Z}^{3}(\mathrm{aq})+3 \mathrm{e}^{-} \longrightarrow \mathrm{Z}(\mathrm{s})$ & 1.52 \\ Identify the strongest oxidizing agent. X $Y$ $\mathrm{X}^{+}$ Z $\mathrm{Y}^{2+}$ $Z^{3+}$ Identify the strongest reducing agent. $Z^{3+}$ $Y$ Z $\mathrm{Y}^{2+}$ $\mathrm{X}^{+}$ $x$ Identify the weakest oxidizing agent. $X$ $Y$ Z $\mathrm{X}^{+}$ $\mathrm{Y}^{2+}$ $Z^{3+}$ Identify the weakest reducing agent. X $Y$ $\mathrm{X}^{+}$ $z^{3+}$ $\mathrm{Y}^{2+}$ Z

Solution

Solution Steps

Step 1: Understanding Oxidizing and Reducing Agents

Oxidizing agents gain electrons and are reduced in the process. The stronger the oxidizing agent, the higher its standard reduction potential $ E^{\circ} $.

Reducing agents lose electrons and are oxidized in the process. The stronger the reducing agent, the lower its standard reduction potential $ E^{\circ} $.

Step 2: Identifying the Strongest Oxidizing Agent

The strongest oxidizing agent will have the highest standard reduction potential $ E^{\circ} $.

From the table:

$ \mathrm{X}^{+}(\mathrm{aq}) + \mathrm{e}^{-} \rightarrow \mathrm{X}(\mathrm{s}) $ has $ E^{\circ} = 0.84 \, \text{V} $
$ \mathrm{Y}^{2+}(\mathrm{aq}) + 2 \mathrm{e}^{-} \rightarrow \mathrm{Y}(\mathrm{s}) $ has $ E^{\circ} = -1.17 \, \text{V} $
$ \mathrm{Z}^{3+}(\mathrm{aq}) + 3 \mathrm{e}^{-} \rightarrow \mathrm{Z}(\mathrm{s}) $ has $ E^{\circ} = 1.52 \, \text{V} $

The highest $ E^{\circ} $ is 1.52 V for $ \mathrm{Z}^{3+} $.

$\boxed{\text{The strongest oxidizing agent is } Z^{3+}}$

Step 3: Identifying the Strongest Reducing Agent

The strongest reducing agent will have the lowest standard reduction potential $ E^{\circ} $.

From the table:

$ \mathrm{X}^{+}(\mathrm{aq}) + \mathrm{e}^{-} \rightarrow \mathrm{X}(\mathrm{s}) $ has $ E^{\circ} = 0.84 \, \text{V} $
$ \mathrm{Y}^{2+}(\mathrm{aq}) + 2 \mathrm{e}^{-} \rightarrow \mathrm{Y}(\mathrm{s}) $ has $ E^{\circ} = -1.17 \, \text{V} $
$ \mathrm{Z}^{3+}(\mathrm{aq}) + 3 \mathrm{e}^{-} \rightarrow \mathrm{Z}(\mathrm{s}) $ has $ E^{\circ} = 1.52 \, \text{V} $

The lowest $ E^{\circ} $ is -1.17 V for $ \mathrm{Y} $.

$\boxed{\text{The strongest reducing agent is } Y}$

Step 4: Identifying the Weakest Oxidizing Agent

The weakest oxidizing agent will have the lowest standard reduction potential $ E^{\circ} $.

From the table:

$ \mathrm{X}^{+}(\mathrm{aq}) + \mathrm{e}^{-} \rightarrow \mathrm{X}(\mathrm{s}) $ has $ E^{\circ} = 0.84 \, \text{V} $
$ \mathrm{Y}^{2+}(\mathrm{aq}) + 2 \mathrm{e}^{-} \rightarrow \mathrm{Y}(\mathrm{s}) $ has $ E^{\circ} = -1.17 \, \text{V} $
$ \mathrm{Z}^{3+}(\mathrm{aq}) + 3 \mathrm{e}^{-} \rightarrow \mathrm{Z}(\mathrm{s}) $ has $ E^{\circ} = 1.52 \, \text{V} $

The lowest $ E^{\circ} $ is -1.17 V for $ \mathrm{Y}^{2+} $.

$\boxed{\text{The weakest oxidizing agent is } \mathrm{Y}^{2+}}$