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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

The reduction potential values of $A, B, C$ are $0.34 \ V, -0.80 \ V, -0.46 \ V$ respectively. What will be the order of the strength of the reducing agent?

Zinc can be coated on iron to produce galvanized iron,but the reverse is not possible. This is because:

Assertion : $Cu^{2+}$ ions get reduced more easily than $H^{+}$ ions.
Reason : Standard electrode potential of copper is $0.34 \ V$.

The standard reduction potential for $Li^{+}/Li$,$Zn^{2+}/Zn$,$H^{+}/H_2$ and $Ag^{+}/Ag$ is $-3.05$,$-0.762$,$0.00$ and $+0.80 \ V$. Which of the following has the highest reducing capacity?

Given
$E^o_{Cl_2/Cl^-} = 1.36 \ V,$
$E^o_{Cr^{3+}/Cr} = -0.74 \ V,$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V,$
$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
Among the following,the strongest reducing agent is:

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