Match each standard reduction half-reaction on the left with its corresponding property re… — JAMB UTME

Match each standard reduction half-reaction on the left with its corresponding property regarding reducing/oxidizing strength or reaction spontaneity on the right. Which pairs correctly match each half-reaction with its chemical behavior?

$\text{Zn}^{2+}(aq) + 2e^- \rightarrow \text{Zn}(s) \quad (E^\circ = -0.76\text{ V})$ Stronger reducing agent than hydrogen; metal spontaneously displaces $\text{H}_2$ from dilute acids
$\text{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s) \quad (E^\circ = +0.80\text{ V})$ Species whose metal form is less reactive than hydrogen and cannot displace $\text{H}_2$ from dilute acids
$\text{2H}^+(aq) + 2e^- \rightarrow \text{H}_2(g) \quad (E^\circ = 0.00\text{ V})$ Standard reference half-cell assigned an electrode potential of zero
$\text{F}_2(g) + 2e^- \rightarrow 2\text{F}^-(aq) \quad (E^\circ = +2.87\text{ V})$ Strongest oxidizing agent among the listed species, reduced most readily

Cevap

The correct pairings match

\text{Zn}^{2+}/\text{Zn}

with being a stronger reducing agent than hydrogen that displaces

\text{H}_2

from acid,

\text{Ag}^+/\text{Ag}

with a metal that cannot displace hydrogen,

\text{2H}^+/\text{H}_2

with the standard reference electrode, and

\text{F}_2/\text{F}^-

with the strongest oxidizing agent.

Zinc has a negative reduction potential and displaces hydrogen from acid; silver has a positive reduction potential and cannot displace hydrogen; hydrogen serves as the reference potential at zero; fluorine gas possesses the highest positive reduction potential, functioning as the strongest oxidizing agent.

Adım Adım Çözüm

Examine standard reduction potential (

E^\circ

) values

Higher positive values indicate a stronger tendency to gain electrons (stronger oxidizing agent). Negative values indicate that the reduced form easily loses electrons (stronger reducing agent).

Standard reduction potentials dictate relative oxidizing/reducing strength and reaction feasibility.

Relate

E^\circ

values to hydrogen displacement and spontaneity

Metals with

E^\circ < 0.00\text{ V}

(like

\text{Zn}

) spontaneously displace

\text{H}_2

from acids. Metals with

E^\circ > 0.00\text{ V}

(like

\text{Ag}

) do not.

A reaction is spontaneous when the overall standard cell potential

E^\circ_{\text{cell}}

is positive.

Match each half-reaction to its appropriate description

\text{Zn}^{2+}/\text{Zn}

matches with displacing

\text{H}_2

;

\text{Ag}^+/\text{Ag}

matches with inability to displace

\text{H}_2

;

\text{2H}^+/\text{H}_2

matches with the zero reference electrode;

\text{F}_2/\text{F}^-

matches with the strongest oxidizing agent.

Each standard reduction potential maps directly to these electrochemical behaviors.

Anahtar Kavram

Electrochemical Series and Reaction Spontaneity

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