Respuesta :

Answer: The correct answer is Option b.

Explanation:

Reducing agents are defined as the agents which help the other substance to get reduced and itself gets oxidized. They undergo oxidation reaction.

[tex]X\rightarrow X^{n+}+ne^-[/tex]

For determination of reducing agents, we will look at the oxidation potentials of the substance. Oxidation potentials can be determined by reversing the standard reduction potentials.

For the given options:

  • Option a:  [tex]Ag^+[/tex]

This ion cannot be further oxidized because +1 is the most stable oxidation state of silver.

  • Option b:  [tex]Pb[/tex]

This metal can easily get oxidized to [tex]Pb^{2+}[/tex] ion and the standard oxidation potential for this is 0.13 V

[tex]Pb\rightarrow Pb^{2+}+2e^-;E^o_{(Pb/Pb^{2+})}=+0.13V[/tex]

  • Option c:  [tex]H_2[/tex]

This metal can easily get oxidized to [tex]H^{+}[/tex] ion and the standard oxidation potential for this is 0.0 V

[tex]H_2\rightarrow 2H^++2e^-;E^o_{(H_2/H^{+})}=0.0V[/tex]

  • Option d:  [tex]Ag[/tex]

This metal can easily get oxidized to [tex]Ag^{+}[/tex] ion and the standard oxidation potential for this is -0.80 V

[tex]Ag\rightarrow Ag^{+}+e^-;E^o_{(Ag/Ag^{+})}=-0.80V[/tex]

  • Option e:  [tex]Mg^{2+}[/tex]

This ion cannot be further oxidized because +2 is the most stable oxidation state of magnesium.

By looking at the standard oxidation potential of the substances, the substance having highest positive [tex]E^o[/tex] potential will always get oxidized and will undergo oxidation reaction. Thus, considered as strong reducing agent.

From the above values, the correct answer is Option b.

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