Given: `E^(@) (Sn^(2+)Sn^(4+)|Pt) = -0.15V, E^(@) (Hg_(2)^(2+)|Hg ^(2+))=-0.92 V and E^(@) (Pb^(2+), H^(+)|PbO_(2)) = -1.67V` Based on this data, which of the following statements is correct?

Options

A. `Sn^(4+)` is a stronger oxidizing agent than `Pb^(4+)`
B. `Sn^(2+)` is a stronger reducing agent than `Hg_(2)^(2+)`
C. `Hg^(2+)` is a stronger oxidizing agent than `Pb^(4+)`
D. `Pb^(2+)` is a stronger reducing agent than `Sn^(2+)`

Answer

B

Explanation

Larger the reduction potential, larger the oxidation tendency of the ion being reduced. Hence, the oxidizing tendency follows the order `Pb^(4+)gtH^(2+)ggtSn^(4+)`.. Lesser the reduction potential, larger the reduction tendency of the ion formed in the reduction reaction. 40. B Hence, the reducing tendency follows the order `Sn^(2+)gtHg^(2+)gtPb^(2+)`