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(A) The strength of a reducing agent is inversely proportional to its standard reduction potential $(E^o)$.The lower (more negative) the standard redu

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$Zn_{(s)}$

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(A) The strength of a reducing agent is inversely proportional to its standard reduction potential $(E^o)$.The lower (more negative) the standard reduction potential,the easier it is for the species to undergo oxidation,making it a stronger reducing agent.Comparing the given $E^o$ values:$Zn^{2+}/Zn = -0.76\,V$$Cr^{3+}/Cr = -0.74\,V$$H^+/H_2 = 0.00\,V$$Fe^{3+}/Fe^{2+} = +0.77\,V$Since $-0.76\,V$ is the most negative value,$Zn_{(s)}$ has the highest tendency to lose electrons and act as the strongest reducing agent among the given options.

Similar Questions

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If $Cu^{2+} + 2e^{-} \rightarrow Cu, E^{0} = 0.337 \ V$ and $Cu^{2+} + e^{-} \rightarrow Cu^{+}, E^{0} = 0.153 \ V$,then for the reaction $Cu^{+} + e^{-} \rightarrow Cu$,$E^{0}_{cell} =$ .............. $V$.

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