Consider the cell potentials E0Mg2- -Mg -2-37 V and E0Fe3- -Fe - - 0-04 V- The best reducing agent would be-

Given the standard reduction potentials:

Zn²⁺/Zn = - 0.74 V, Cl₂/Cl^- = 1.36 V, H⁺/1/2H₂ = 0 V and Fe³⁺/Fe²⁺ = 0.77 V.
The order of increasing strength as reducing agent is

Q. For the given electrochemical cells :

Cell 1:

E_{F e^{2 +} (a q) / F e (s)}^{\circ} = - 0.44 V

E_{H^{+} (a q) / H_{2} (g)}^{\circ} = 0 V

Cell 2:

E_{M g^{2 +} (a q) / M g (s)}^{\circ} = - 2.37 V

E_{H^{+} (a q) / H_{2} (g)}^{\circ} = 0 V

Choose the correct option:

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Consider the cell potentials E0Mg2+|Mg=−2.37 V and E0Fe3+|Fe=−0.04 V. The best reducing agent would be:

The correct option is C MgSince the reduction potential E0Mg2+|Mg is lower than E0Fe3+|Fe, it will be best reducing agent.The higher the negative value of the standard reduction potential of metal ion, the higher will be its reducing property.Hence option C is correct.

Consider the cell potentials $E_{M g^{2 +} | M g}^{0} = - 2.37$ V and $E_{F e^{3 +} | F e}^{0} = - 0.04$ V. The best reducing agent would be: