The standard potentials at 298 K areE∘Zn2+∣Zn=−0.763V, E∘Cr3+∣Cr=−0.41VE∘H+H2Pt=0.00   and  E∘Fe3+,Fe2+∣Pt=0.770VWhich is the strongest reducing agent?

# The standard potentials at 298 K are${E}^{\circ }\left({\mathrm{H}}^{+}\left|{\mathrm{H}}_{2}\right|\mathrm{Pt}\right)=0.00$   and  ${E}^{\circ }\left({\mathrm{Fe}}^{3+},{\mathrm{Fe}}^{2+}\mid \mathrm{Pt}\right)=0.770\mathrm{V}$Which is the strongest reducing agent?

1. A

Zn(s)

2. B

Cr (s)

3. C

${\mathrm{H}}_{2}\left(\mathrm{g}\right)$

4. D

${\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)$

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### Solution:

The smaller the value of reduction potential, lesser the reduction tendency of the ion and larger the oxidation tendency of the corresponding metal. Larger oxidation tendency implies stronger reducing agent.

A reducing agent is a substance that undergoes oxidation to a higher valency state in a redox reaction and loses electrons to other substances in the process. In an oxidation-reduction process, a reducing agent is one of the reactants that reduces another reactant by discharging electrons onto it.  +91

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