Answer 1

The following reactions are involved when Cr²⁺ and Fe²⁺ act as reducing agents.

`Cr^(2+) -> Cr^(3+)Fe^(2+) -> Fe^(3+)`

The  `E_((Cr^(3+))/(Cr^(2+)))^@` value is -0.14 V and `E_(" "(Fe^(3+))/(Fe^(2+)))^@` is + 0.77 V. This means that Cr²⁺ can be easily oxidized to Cr³⁺, but Fe²⁺ does not get oxidized to Fe³⁺ easily. Therefore, Cr²⁺ is a better reducing agent that Fe³⁺.

Answer 2

Cr²⁺ is a stronger reducing agent than Fe²⁺. This is because E°(Cr³⁺/Cr²⁺) is negative (- 0.41V) whereas E°(Fe³⁺/Fe²⁺) is positive (+ 0.77 V). Thus, Cr²⁺ is easily oxidised to Fe³⁺ but Fe²⁺ cannot be easily oxidised to Fe³⁺.