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(D) The strength of a reducing agent is inversely proportional to its standard reduction potential $(E^0_{red})$. $A$ lower (more negative) reduction

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$Zn$

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(D) The strength of a reducing agent is inversely proportional to its standard reduction potential $(E^0_{red})$. $A$ lower (more negative) reduction potential indicates that the substance is more easily oxidized and is therefore a stronger reducing agent. Comparing the given values: $1. E^0_{MnO_4^-/Mn^{2+}} = 1.51 	ext{ V}$ $2. E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 	ext{ V}$ $3. E^0_{Br_2/Br^{-}} = 1.09 	ext{ V}$ $4. E^0_{Zn^{2+}/Zn} = -0.76 	ext{ V}$ Since $E^0_{Zn^{2+}/Zn}$ has the lowest value $(-0.76 	ext{ V})$,$Zn$ is the strongest reducing agent.

On the basis of the following electrode potentials,which one is the strongest reducing agent?
$E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$,$E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$,$E^0_{Br_2/Br^{-}} = 1.09 \text{ V}$,$E^0_{Zn^{2+}/Zn} = -0.76 \text{ V}$

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On the basis of the following electrode potentials,which one is the strongest reducing agent? $E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$,$E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$,$E^0_{Br_2/Br^{-}} = 1.09 \text{ V}$,$E^0_{Zn^{2+}/Zn} = -0.76 \text{ V}$