The equivalent weight of Ferrous Oxalate is $\frac{molecularweight}{n}.$ When it acts as reluctant, n is

The value of n when Ferrous Oxalate (FeC₂O₄) acts as a reductant is:

n = 3

Detailed Explanation:

1. Ferrous Oxalate (FeC₂O₄): Ferrous Oxalate contains iron in the +2 oxidation state (Fe²⁺) and oxalate ions (C₂O₄^2-). In a redox reaction, ferrous ions (Fe²⁺) can be oxidized to ferric ions (Fe³⁺).
2. Equivalent weight formula: The equivalent weight of a substance is given by the formula: 
   Equivalent weight = (Molecular weight) / n
   Where n represents the number of electrons transferred during the redox reaction.
3. In the case of Ferrous Oxalate: When ferrous ions (Fe²⁺) in Ferrous Oxalate are oxidized to ferric ions (Fe³⁺), each molecule of Ferrous Oxalate donates 3 electrons (one for each Fe²⁺ ion and the two electrons involved in the reduction of oxalate ions to CO₂). Hence, n = 3 for this reaction.

Concept:

• The equivalent weight of a compound is determined by the number of electrons it donates or accepts in a redox reaction, denoted by n.
• For Ferrous Oxalate, the total number of electrons donated during the reaction is 3 (1 from Fe²⁺ to Fe³⁺ and 2 from oxalate ions), so n = 3.